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Published byJustina Morris Modified over 6 years ago

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**#1) If 0.20 bushel is 1 dozen apples and a dozen **

apples has a mass of 2.0 kg, what is the mass of 0.50 bushel of apples? ____2.0 Kg___ 1 dozen apples .20 bushel 1 dozen apples 2.0 Kg 1 dozen apples 1 dozen apples .2 bushel 0.5 bushel l X X = 5.0 Kg

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**#2 Assume 2.0 kg of apples is 1 dozen and**

that each apple has 8 seeds. How many apple seeds are in 14 kg of apples? 8 seeds 1 apple 1 dozen apples 2.0 kg 12 apples 1 dozen 1 dozen 2.0 kg 14 kg apple 1 X X 8 seeds 1 apple 672 seeds X =

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**3) How many moles is 2.80 x 1023 atoms of silicon?**

4.65 mol Si

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**representative particles of bromine?**

4) How many moles is 2.17 x 1023 representative particles of bromine? the representative particle for bromine is Br2 1 mole 6.02 x 1024 part. 2.17 x 1023 part. 1 X .360 mol Br2

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**5) How many atoms are in 1.14 mol SO3**

1 molecule 1.14 mole 1 6.02 molecules 1 mole X X 2.75 x atoms

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**6) How many moles are in 4.65 x 1024 molecules of NO2 SO3 1 mole**

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**To find the molar mass simply add up the atomic masses of the atoms **

#7 Find the molar mass of PCl3 To find the molar mass simply add up the atomic masses of the atoms in the molecule (4 atoms total here) P =30.97amu Cl=35.4amu = g

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**#8 What is the mass of 1.00 mol of sodium hydrogen carbonate?**

NaHCO3 consists of 6 atoms total in one formula unit. Adding them up you get: Na = 23.0g/mol H = 1g/mol C = 12.0g/mol O= 16g/mol = 84.0 g

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**#9 What are three ways to measure the**

amount of something? simple counting volume weight

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**#10 Describe the relationship between**

Avogadro’s number and one mole of any substance. Avogadro’s number is the number of representative particles you have in one mole which is 6.02 x 1023

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**#11 How is the atomic mass of an element**

related to the molar mass of the element? The atomic mass is the number of grams of an element that you need to have exactly one mole of that substance ie x 1023 particles.

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**#12 How can you calculate the mass of a**

mole of a compound? You add up the individual atomic masses of each atom within the formula of the compound. example: H2O is 1g+1g+16g = 18 grams 1 mole

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#13 How many moles is 1.50 X 1023 molecules NH3? 1 mole NH3 6.02 x 1023 molecules 1.50 X 1023 molecules NH3 1 X 2.49 x 10-1 mole NH3

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**#14 How many atoms are in 1.75 moles**

of CHCl3? 6.02 x 1023 atoms 1 mole 1.75 moles of CHCl3 1 X 5.27 x 1024 atoms

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**#15 What is the molar mass of CaSO4?**

= g/mol

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