Topic 1 – Quantitative Chemistry
Topic 1.1 – The Mole Concept and Avogadro’s Constant
1. How many moles of Cu are present in 35.4 g of Cu? How many atoms of Cu are present in 35.4 g
of Cu? 0.557 mol
2. What is the mass (in grams) of 1.20x1024 molecules of glucose (C6H12O6)? 358 g
3. What is the mass of 4.56 mols of NaCl? 267g
4. How many molecules are there in 450 grams of Na2SO4 ? 1.9x1024 molecules
5. How many grams are there in 3.3 x 1023 molecules of N2I6 ? 430g
6. How many moles are there in 22.50 grams of K2SO4 ?
a. How many Atoms? [in 22.50 grams of K2SO4] 0.1291mol
b. How many Formula units? [22.50 grams of K2SO4] 7.77x1022 atoms
Topic 1.2 – Formulas
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1.
2.
3.
4.
5.
Define the terms: relative atomic mass (Ar), relative molecular mass (Mr),
Ar is the weighted mean of all naturally occurring isotopes of the element, relative to carbon-12
Mr is the mass of a molecule. Calculated by adding each atoms relative atomic mass together
Calculate the Molar Mass of calcium phosphate 310.3 g/mol
Calculate the mass percentage of Nitrogen in each compound:
a. N2O 63.65%
b. Sr(NO3)2 13.24%
c. NH4NO3 35.00%
d. HNO3 22.23%
e. NH4 77.62%
f. KNO3 13.86%
Calculate empirical formula of a compound that is 85.6% carbon and 14.4% hydrogen. CH2
Find the empirical formula for the following:
a. 17.5% hydrogen and 82.4% nitrogen NH3
b. 46.3% lithium and 53.7% oxygen Li2O
Page 97 # 17, 18, 19; Page 107 – 109 # 6, 8, 12,13, 14, 22
Topic 1.3 – Chemical Equations
1. Write the balanced reaction for hydrogen gas reacting with oxygen gas 2 H2 + O2  2 H2O
2. How many moles of chlorine is needed to react with 5.0 moles of sodium (without any sodium
left over)? 2 Na + Cl2  2 NaCl 2.5 mol
3. How many grams of chlorine are required to react completely with 5.00 moles of sodium to
produce sodium chloride? 177g
4. Calculate the mass in grams of Iodine required to react completely with 0.50 moles of aluminum
190g
5. Calculate the number of moles of ethane (C2H6) needed to produce 10.0 g of water 0.185g
6. Calculate how many grams of ammonia are produced when you react 2.00g of nitrogen with
excess hydrogen. 2.44g
7. Page 126 – 127 Questions: 1, 3-7
Topic 1.4 - Mass and Gaseous volume relationships in chemical reactions
1. 10.0g of aluminum reacts with 35.0 grams of chlorine gas to produce aluminum chloride.
Which reactant is limiting, which is in excess, and how much product is produced? 43.9g
2. 15.0 g of potassium reacts with 15.0 g of iodine. Calculate which reactant is limiting and
how much product is made 19.6g
3. Page 131 # 23, 24, 25; Page 134 # 27 and 29
4. 20.0 g of HBrO3 is reacted with excess HBr. What is the theoretical yield of Br2? 74.4g;
63.6%
What is the percent yield, if 47.3g is produced? HBrO3 + 5HBr  3H2O + 3 Br2
5. When 35.0 g of Ba(NO3)2 is reacted with excess Na2SO4, 29.8g of BaSO4 is recovered.
Ba(NO3)2 + Na2SO4  BaSO4 + 2NaNO3
Calculate the theoretical yield and the percent yield of BaSO4 31.3g; 95.2%
6. Pg.139 # 31, 33; Pg. 141 # 35
7. A chemical reaction produces 0.0680 mol of oxygen gas. What volume in liters is occupied
by this gas sample at STP? 1.52L
8. A chemical reaction produced 98.0 mL of sulfur dioxide gas at STP. What was the mass of
gas made? 0.280g
9. A chemical reaction produced 3.1 g of CO2 gas. What volume will it have in mL at STP?
1600mL
10. How many moles of gas are in a container with a volume of 2.46 dm3 at STP? 0.110mol
11. Assume all volumes are measured at the same temperature and pressure.
What volume of nitrogen forms when 100 cm3 of ammonia decomposes completely into its
elements. What volume of oxygen is needed to react with 40 cm3 of butane,C4H10 ,and what
volume of carbon dioxide is produced?
50cm3; 260 cm3; 160 cm3
12. Calculate the volume occupied by 4.40g of carbon dioxide at standard temperature and
pressure. 2.24 dm3
13. Calcium reacts with water to produce hydrogen. Calculated the volume of the gas,
measured at STP produced when 0.200g of calcium reacts completely with water?
0.112 dm3