1. What is a Mole?
3.3

2. The Mole contains a LOT of particles! 6.022 × 1023 particles video…

3. The Mole is the SI unit for amount of substance. is abbreviated mol.
is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of C-12.

4. How are Moles Used?
3.3, 8.1, 9.1

5. Moles… are part of every balanced chemical equation
they are the coefficients in front of the chemical formulas

6. Mole Ratios…
are the ratios of the coefficients in the balanced equation

7. Mole Ratios… Examples Given the reaction:
Calcium reacts with hydrochloric acid to form calcium chloride and hydrogen
Translate/balance the equation.
Find the ratio of hydrochloric acid to calcium.

8. Mole Ratios… Examples: Given the reaction:
Hydrogen reacts with oxygen to produce water
Translate/balance the equation.
Find the ratio of oxygen to hydrogen.

9. Molar Mass…
is the mass of one mole of an element or compound with units of grams.

10. Molar Mass…
can be determined from the periodic table - use g with the atomic mass instead of amu.

11. Molar Mass… 1 mole H atoms = _ atoms = _ g
1 mole N atoms = _ atoms = _ g
1 mole S atoms = _ atoms = _ g

12. Molar Mass… 1 mole H atoms = 6.022 x 1023 H atoms = 1.0079 g
1 mole N atoms = x 1023 N atoms = g
1 mole S atoms = x 1023 S atoms = g

13. Molar Mass… Why are there different masses for different elements?
this is due to the varying numbers of protons, neutrons, & electrons in each element

14. Molar Mass…
Examples:
Calculate the molar mass of NaCl. g

15. Molar Mass…
Examples:
Calculate the molar mass of Fe2O3. g

16. Molar Mass…
Examples:
Calculate the molar mass of Mg(OH)2. g

17. Moles & Conversions
3.3 & 10.3
More good

18. Mole Conversions…
use conversion factors to allow us to convert between moles, particles (atoms, molecules, etc.), mass, and volume.
Molar mass
Molar volume
Avagadro’s number

19. Volume
(gases only)
Mole
Mass
Particles

21. Welcome to Mole Island 1 mol = 1 mol = molar mass
in grams
1 mol =
6.022 x 1023 particles
1 mole = 22.4 L
@ STP

22. Mole Conversions… If there are 16 g of S, how many moles are there?
16 g × (1 mol/32.07 g) = 0.50 moles

23. Mole Conversions… How many atoms are in 3.5 moles of Cu?
3.5 moles Cu × (6.022 x 1023 atoms/1 mole) = x 1024 Cu atoms

24. Mole Conversions…
A chemical reaction makes 0.82 moles of O2 gas. What is the volume at STP?
0.82 mol × (22.4 L/1 mol) = 18 L of O2 gas

25. Mole Conversions… Find the mass in grams of 3.50 moles of Cu.
3.50 mol Cu × (63.55 g Cu/1 mol Cu) = 222 g Cu

26. Mole Conversions… How many moles of Ag are in 3.01 x 1023 atoms?
3.01 x 1023 atoms × (1 mole/6.022 x 1023 atoms) = moles Ag

27. Mole Conversions…
A room has a volume of L. How many moles of air would that be (STP)?
4000. L × (1 mol/22.4 L) = 179 moles of air

28. Review of Gases New chap!!

29. The nature of gases… Gases all have common physical properties: Mass
Easily compressible
Take the shape of their container
Can move through other gases
Exert pressure
Pressure depends on temperature

30. The kinetic-molecular theory…
Explains the behavior of gas particles

31. Assumptions of K-M theory…
Gas consists of very small particles, each of which has a mass
Distances separating gas particles are relatively large
Gas particles are in constant, rapid, random motion
Collisions of gas particles with each other or container are perfectly elastic
Average kinetic energy of particles depends only on temperature of the gas
Gas particles exert no force on one another

32. Measuring Gases

33. Measuring gases… 4 variables: Amount of gas (n) Volume (V)
Temperature (T)
Pressure (P)

34. The gas laws… A useful bit of information:
Conditions for STP are 0.00 C and 1.00 atm

35. Combined Gas Law

36. The gas laws…
The combined gas law – relates pressure, volume, and temperature
formula:
(P1V1) = (P2V2)
T1 T2

37. The combined gas law Sample Problem:
The volume of a gas-filled balloon is 30.0 L at 40. C and 153 kPa. What volume will the balloon have at STP?

38. The combined gas law… Sample Problem:
(153 kPa × 30.0 L)/313 K = (101.3 kPa × V2)/273 K
((153 kPa × 30.0 L)/313 K) × (273 K/101.3 kPa) = L

39. The combined gas law… Sample Problem:
A gas occupies a volume of mL at 316 K and 4.89 atm. What volume will it occupy at STP?

40. The combined gas law… Sample Problem:
(4.89 atm × mL)/316 K = (1.00 atm × V2)/273 K
((4.89 atm × mL)/316 K) × (273 K/1.00 atm) = mL

41. Gas Laws Work – due 5/23: Pg 375: #4, 5
Pg : #1, 3, 5a, 23, 29, 31
For #31, change mm Hg to atm