# Mole Problems Solution Guide.

## Presentation on theme: "Mole Problems Solution Guide."— Presentation transcript:

Mole Problems Solution Guide

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min)

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min)

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min)

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min)

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min)

How many water molecules are found in 18.0g water?
6.02x1023 water molecules If you had 6.02x1023 dollar bills you would need to spend \$238 trillion dollars per second for every day of an 80 year life span to spend that many dollars, if you shared it with each person on the planet they would have to spend \$34,000 dollars per second every day of their 80 year life span to spend it all. \$6.02x = \$238,616,184,677,188.51 (80yrs ) (365 d) ( 24hr) ( 60min) (60s ) second ( 1yr ) ( 1 d) ( 1hr ) (1min) In any measurable sample of matter there are too many particles to count directly! Atoms are exceedingly small!!!

One H has a relative mass of ______ amu One C has a relative mass of _______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu H have a relative mass of _____ amu C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of _______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu H have a relative mass of _____ amu C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of ______ amu C have a relative mass of ______ amu H have a relative mass of _____ amu C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of ______ amu H have a relative mass of _____ amu C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of __ amu H have a relative mass of ____ amu C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of __ amu H have a relative mass of 100 amu _ C have a relative mass of ______ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of __ amu H have a relative mass of 100 amu _ C have a relative mass of _ amu H have a relative mass of ______ amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of __ amu H have a relative mass of 100 amu _ C have a relative mass of _ amu H have a relative mass of 1million amu C have a relative mass of ______ amu

One H has a relative mass of __1___ amu One C has a relative mass of ___12__ amu H have a relative mass of _10___ amu C have a relative mass of __ amu H have a relative mass of 100 amu _ C have a relative mass of _ amu H have a relative mass of 1million amu C have a relative mass of 12 million amu

1a) The mass of the sample of carbon is
always ______ more than an equivalent number of hydrogens

Mole Unit Questions 1a) The mass of the sample of carbon is
always _12x__ more than an equivalent number of hydrogens

Mole Unit Question 1 6.02x1023 atoms of hydrogen have a mass of 1.0 g that equals the atomic mass of hydrogen found on the periodic table 6.02x1023 atoms of carbon have a mass of 12.0 g that equals the atomic mass of carbon found on the periodic table

Mole Unit Question 1 6.02x1023 atoms of hydrogen have a mass of 1.0 g that equals the atomic mass of hydrogen found on the periodic table 6.02x1023 atoms of carbon have a mass of 12.0 g that equals the atomic mass of carbon found on the periodic table

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 2. What is the mass of 3.01 x 1023 carbon–12 atoms?
3.01 x is one half of 6.02 x 1023 therefore the mass will be one half of 12 g = 6g 3. What is the mass of x 1023 carbon–12 atoms? 1.51 x is one fourth of 6.02 x 1023 therefore the mass will be one fourth of 12 g = 3g 4. What is the mass of x 1023 carbon–12 atoms? 12.04 x 1023 is twice 6.02 x 1023 therefore the mass will be twice 12 g = 24 g

Questions 2-8 5. What is the mass of 24.01 x 1023 carbon–12 atoms?
24.01 x 1023 is four times 6.02 x 1023 therefore the mass will be four time 12 g = 48g

Questions 2-8 5. What is the mass of 24.01 x 1023 carbon–12 atoms?
24.01 x 1023 is four times 6.02 x 1023 therefore the mass will be four time 12 g = 48g

Questions 2-8 5. What is the mass of 24.01 x 1023 carbon–12 atoms?
24.01 x 1023 is four times 6.02 x 1023 therefore the mass will be four time 12 g = 48g

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Questions 2-8 6. How many carbon atoms are in 36.0 g
36.0g is three times 12.0g therefore there are three times 6.02x1023 C = 18.06x1023C = 1.806x1024 C 7. How many carbon atoms are in 4.0 g 4.0 g is one third of 12.0g therefore one third of 6.02x1023 C = 2.01x1023C 8. How many carbon atoms are in 1.0 g 1.0 g is one twelfth of 12.0g therefore one twelfth x1023 C = 5.01x1022 C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question 6.02x1023 C = 12.0 g C 1.0 x106 C = x
Cross multiply 1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C = 1.99x10-17g C

Bonus Question Cross multiply
1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C 1.0 x106 C ( g C ) = 1.99x10-17g C (6.02x1023 C )

Bonus Question Cross multiply
1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C 1.0 x106 C ( g C ) = 1.99x10-17g C (6.02x1023 C )

Bonus Question Cross multiply
1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C 1.0 x106 C ( g C ) = 1.99x10-17g C (6.02x1023 C )

Bonus Question Cross multiply
1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C 1.0 x106 C ( g C ) = 1.99x10-17g C (6.02x1023 C )

Bonus Question Cross multiply
1.0 x106 C multiplied by 12.0 g then divided by 6.0x1023 C 1.0 x106 C ( g C ) = 1.99x10-17g C (6.02x1023 C )

6.02 x 1023 = P.T. grams 9. How many silver atoms are in 25.0 grams of

6.02 x 1023 = P.T. grams 9. How many silver atoms are in 25.0 grams of
25.0g Ag

6.02 x 1023 = P.T. grams 9. How many silver atoms are in 25.0 grams of
25.0g Ag x 1023 Ag =

6.02 x 1023 = P.T. grams 9. How many silver atoms are in 25.0 grams of
25.0g Ag x 1023 Ag = 107.9g

6.02 x 1023 = P.T. grams 9. How many silver atoms are in 25.0 grams of
25.0g Ag x 1023 Ag =1.39x1023 Ag 107.9Ag

6.02 x 1023 = P.T. grams 10. What is the mass of 1.00 x 109 silver
atoms? 1.00 x 109 Ag

6.02 x 1023 = P.T. grams 10. What is the mass of 1.00 x 109 silver
atoms? 1.00 x 109 Ag ( g Ag ) =

6.02 x 1023 = P.T. grams 10. What is the mass of 1.00 x 109 silver
atoms? 1.00 x 109 Ag ( g Ag ) = (6.02 x 1023 Ag )

6.02 x 1023 = P.T. grams 10. What is the mass of 1.00 x 109 silver
atoms? 1.00 x 109 Ag ( g Ag ) = 1.79 x g Ag (6.02 x 1023 Ag )

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 11. What is the mass of 2.00 x 1023 gold
atoms? 2.00 x 1023 Au ( g Au ) = 65.4 g Au (6.02 x 1023 Au ) 12. How many gold atoms are in 100 grams of gold? 100g Au x 1023 Au = 3.06 X1023 Au 197.0 g Au

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 13. What is the mass x platinum atoms? 2.00 x Pt ( g Pt ) = 648 g Pt (6.02 x 1023 Pt ) 14. What is the mass of 2.00 x silicon atoms? 2.00 x 1022 Si ( g Si ) = .93 g Si (6.02 x 1023 Si )

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 15. How many silicon atoms are in 12.0 grams of silicon atoms? 12g Si x 1023 Si = 2.57X1023 Si 28.1g Si 16. How many lead atoms are in 12.0 grams of lead? 12.0g Pb x 1023 Pb = 3.49 X1022 Pb 207.2 g Pb

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 ) )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 17. What is the mass of 2.0 x109 Pb atoms?
2.0 x109 Pb g Pb =6.88x10-13g Pb 6.02 x 1023 Pb 18. What is the mass of 1.51 x1023 C6H12O6? 1.51 x1023 C6H12O6 (180 g C6H12O6 )= 45.0g C6H12O6 (6.02 x 1023 C6H12O6)

6.02 x 1023 = P.T. grams 19. How many copper (II) nitrate are in 454g Cu(NO3)2 454g Cu(NO3) x 1023 Cu(NO3)2 =1.46x1024 Cu(NO3)2 187.5g Cu(NO3)2

6.02 x 1023 = P.T. grams 19. How many copper (II) nitrate are in 454g Cu(NO3)2 454g Cu(NO3) x 1023 Cu(NO3)2 =1.46x1024 Cu(NO3)2 187.5g Cu(NO3)2

6.02 x 1023 = P.T. grams 19. How many copper (II) nitrate are in 454g Cu(NO3)2 454g Cu(NO3) x 1023 Cu(NO3)2 =1.46x1024 Cu(NO3)2 187.5g Cu(NO3)2

6.02 x 1023 = P.T. grams 19. How many copper (II) nitrate are in 454g Cu(NO3)2 454g Cu(NO3) x 1023 Cu(NO3)2 =1.46x1024 Cu(NO3)2 187.5g Cu(NO3)2

6.02 x 1023 = P.T. grams 19. How many copper (II) nitrate are in 454g Cu(NO3)2 454g Cu(NO3) x 1023 Cu(NO3)2 =1.46x1024 Cu(NO3)2 187.5g Cu(NO3)2

Mole Concept 6.02 x 1023 is known as _____________________ number.
6.02 x 1023 particles is known as __________of particles just as 12 particles is known as a _______ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or ___________ of those particle. __________ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as __________of particles just as 12 particles is known as a _______ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or ___________ of those particle. __________ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as _1mole__of particles just as 12 particles is known as a _______ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or ___________ of those particle. __________ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as _1mole__of particles just as 12 particles is known as a _dozen__ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or ___________ of those particle. __________ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as _1mole__of particles just as 12 particles is known as a _dozen__ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or __1mole__ of those particle. __________ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as _1mole__of particles just as 12 particles is known as a _dozen__ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or __1mole__ of those particle. ___P.T.____ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 ___________ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept 6.02 x 1023 is known as ___Avogadro’s___ number.
6.02 x 1023 particles is known as _1mole__of particles just as 12 particles is known as a _dozen__ The mass of 1 particle in atomic mass units (amu) is equivalent to the mass of 6.02 x of those particles or __1mole__ of those particle. ___P.T.____ g = 1 mole of particles = 6.02 x 1023 particles atomic mass / molecular mass / formula mass 12 __12.0____ g C = 1.00 moles of C = 6.02 x 1023 C atoms 6

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
20. What is the mass of 2 moles C? 2 mol C ( 12.0g C ) = 24.0g C ( 1mol C ) 21. What is the mass of 7.5x1020C? 7.5x1020C ( 12.0g C ) = .015 g C ( 6.02x1023C)

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
22. How many moles of carbon are in 1.806x1025 C atom sample? 1.806x1025 C(1mole C ) = 30 moles C (6.02x1023 C) 23. How many atoms of carbon are in 100g C? 100gC ( 6.02x1023C) = 5.04x1024 C atoms ( 12.0g C )

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
25. How many atoms of carbon are in .750 mole sample? .750 mole C ( 6.02 x1023 C) = 4.52 x1023 C 1mole C

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
25. How many atoms of carbon are in .750 mole sample? .750 mole C ( 6.02 x1023 C) = 4.52 x1023 C 1mole C

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
25. How many atoms of carbon are in .750 mole sample? .750 mole C ( 6.02 x1023 C) = 4.52 x1023 C 1mole C

Mole Concept II 6.02 x 1023 = P.T. grams = 1.0 mole
25. How many atoms of carbon are in .750 mole sample? .750 mole C ( 6.02 x1023 C) = 4.52 x1023 C 1mole C

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams 26. What is the mass of 3.50 moles of C2H5OH?
3.50 mole C2H5OH g C2H5OH=161 g C2H5OH 1mole C2H5OH 27. How many molecules are in .250 mole of C2H5OH? .250 mole C2H5OH 6.02 x 1023 C2H5OH= 1.51 X1023

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 28. How many moles of C2H5OH are in a 1.0x10 3 molecule sample of C2H5OH? 1.00 x 103 C2H5OH 1mole C2H5OH = 1.67x10-21moles x 1023 C2H5OH 29. How many moles of C2H5OH are in 12.0 grams of C2H5OH? 12.0 gC2H5OH 1mole C2H5OH= .26 moles C2H5OH 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 30. What is the mass of 2.50 moles of C2H5OH? 2.50 mole C2H5OH 46.0g C2H5OH = 115 g C2H5OH 1mole C2H5OH 31. How many molecules are found in 454 g C2H5OH 454 gC2H5OH 6.02 X C2H5OH= 5.94X10 24 46.0 g C2H5OH

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 32. How many moles are in 0.10g Ca(NO3)2 ? 0.10 g Ca(NO3)2 1mole Ca(NO3)2 = mol Ca(NO3)2 164.1g Ca(NO3)2 33. What is the mass of .125 moles Ca(NO3)2? .125 moles Ca(NO3) g Ca(NO3)2 =20.5 g Ca(NO3)2 1 mole Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 34. How many units are in 454g Ca(NO3)2? 454g Ca(NO3) X Ca(NO3)2 = 1.67x1024 Ca(NO3)2 164.1g Ca(NO3)2 35. What is the mass of .50 moles Ca(NO3)2? .50 moles Ca(NO3)2(164.1g Ca(NO3)2=82.1g Ca(NO3)2 (1mol Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

6.02 x 1023 = P.T. grams = 1.0 mole 36. How many units are in .250 mol Ca(NO3)2? .250 mole Ca(NO3)2 6.02x1023 Ca(NO3)2 =1.51x1023 Ca(NO3)2 1mole Ca(NO3)2 37. How many moles are in 1.0x109 Ca(NO3)2? 1.0x109 Ca(NO3)2 ( 1mole Ca(NO3)2= 1.66x10-15 mol 6.02x1023 Ca(NO3)2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical Formula Extra Credit
50 g S 50 g O 50g S ( 1mole S) = 1.56 mol S1.0 ( 32 g S ) 50 g O ( 1 mol O ) = 3.13 mol O2.0 ( 16 g O ) SO2

Empirical formula Count the number of particles of each element by determining the number of moles of each element Divide by the smallest number of moles in order to determine the simplest whole number ratio that the elements combine in to form the compound If the ratios are not whole numbers multiply each ratio by a common factor until they are whole number ratios

Empirical formula Count the number of particles of each element by determining the number of moles of each element Divide by the smallest number of moles in order to determine the simplest whole number ratio that the elements combine in to form the compound If the ratios are not whole numbers multiply each ratio by a common factor until they are whole number ratios

Empirical formula Count the number of particles of each element by determining the number of moles of each element Divide by the smallest number of moles in order to determine the simplest whole number ratio that the elements combine in to form the compound If the ratios are not whole numbers multiply each ratio by a common factor until they are whole number ratios

Empirical formula Count the number of particles of each element by determining the number of moles of each element Divide by the smallest number of moles in order to determine the simplest whole number ratio that the elements combine in to form the compound If the ratios are not whole numbers multiply each ratio by a common factor until they are whole number ratios

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula A) 35.6g Co and 64.4 g Cl
35.6gCo(1mole Co)=.603 mol Co1.0 (59.0gCo ) .603 64.4gCl ( 1mole Cl)=1.81 mol Cl3.0 ( 35.5 g Cl) .603 CoCl3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula B) CoCl2 C) 52.9gAl and 47.1gO
52.9gAl(1mole Al)= 1.96 mol Al1.0 (27.0g Al ) 1.96 47.1 gO ( 1mole O)=2.94 mol O1.5 ( g O) 1.96 Al1.0O1.5 x 2 = Al2O3

Empirical Formula D) MgO E) 2.83gK, .435g C, 1.735 g O
2.83 g K ( 1 mole K ) = mole K2 ( 39.1 g K ) .435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g O ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula E) 2.83gK, .435g C, 1.735 g O
2.83 g K ( 1 mole K ) = mole K2 ( 39.1 g K ) .435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g O ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula E) 2.83 g K ( 1 mole K ) = .0724 mole K2
.435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g C ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula E) 2.83 g K ( 1 mole K ) = .0724 mole K2
.435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g C ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula E) 2.83 g K ( 1 mole K ) = .0724 mole K2
.435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g C ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula E) 2.83 g K ( 1 mole K ) = .0724 mole K2
.435 g C ( 1 mole C ) = mole C ( g C ) 1.735 g C ( 1 mole O ) = .108 mole O3 ( g O )

Empirical Formula F) ZnSO3 G) CaC2O4 H) NaCN I) Al2S3O12  Al2(SO4)3
J) Fe2S3O12  Fe2(SO4)3 K) MgCl2O8  Mg(ClO4)2

Similar presentations