Download stoich practice problems sp11

Chemistry Review Packet
Name:
Molar Mass
1. CaCl2
2. HNO3
3. C8H10N4O2
4. Al2(SO4)3
5. Zn (NO3)2
Formula Writing
6. sodium phosphate
7. ammonium carbonate
8. aluminum chromate
9. calcium hydroxide
10. iron (II) fluoride
Period:
Date:
Equation Writing and Balancing
11. Magnesium chloride is the product of a reaction between magnesium and chlorine.
12. Copper (II) hydroxide and potassium sulfate are produced when potassium hydroxide
reacts with copper (II) sulfate.
13. Aluminum nitrate + sodium hydroxide -----> aluminum hydroxide + sodium nitrate
14. Iron (III) oxide + carbon monoxide -----> iron + carbon dioxide
15. Hydrogen chloride reacts with potassium hydroxide to produce water and potassium
chloride.
Mole Conversions
16. 12.4 moles of CO2 = ? grams
17. 3.7 moles of MgCl2 = ? grams
18. 14 grams of PbO = ? moles
19. 19 grams of HCl = ? moles
20. 22 moles of NH4C2H3O2 = ? grams
Stoichiometry
**YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND
COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.**
BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS 5 – 14:
1. ____ Al + ____ O2 → ____ Al2O3
2. ____ Cu + ____ AgNO3 → ____ Ag + ____ Cu(NO3)2
3. ____ Zn + ____ HCl → ____ ZnCl2 + ____ H2
4. ____ Fe + ____ Cl2 → ____ FeCl3
PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS:
5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How
many moles of HCl are required to produce 7.50 moles of ZnCl2?
6. Copper metal reacts with silver nitrate to form silver and copper(II) nitrate. How
many grams of copper are required to form 250 g of silver?
7. When aluminum is burned in excess oxygen, aluminum oxide is produced. How
many grams of oxygen are required to produce 0.75 moles of Al2O3?
8. How many grams of iron(III) chloride are produced when 15.3 g of iron react with
excess chlorine gas?
9. Copper metal reacts with silver nitrate to form silver and copper(II) nitrate. How
many moles of silver will be produced from 3.65 moles of silver nitrate?
10. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas.
How many milliters of 3.00M HCl are required to react with 12.35 g of zinc?
11. How many grams of iron are needed to react with 31.0 L of chlorine gas at STP
to produce iron(III) chloride?
12. When 9.34 g of zinc react with excess hydrochloric acid how many grams of zinc
chloride will be produced?
13. How many liters of oxygen gas at STP are required to react with 65.3 g of
aluminum in the production of aluminum oxide?
14. Copper reacts with silver nitrate to form silver and copper(II) nitrate. How many
grams of copper are required to react with 50.0 mL of 8.0M AgNO3?
15. Nickel nitrate and potassium carbonate react to form nickel carbonate and
potassium nitrate. How many milliliters of 0.55M Ni(NO3)2 are needed to react
with 85 mL of 0.25M K2CO3? First, write a balanced equation.
16. Zinc metal reacts with chromium(III) nitrate in a single replacement reaction.
How many grams of zinc are required to react with 425 mL of 0.25M Cr(NO3)3?
First, write a balanced equation.
PERFORM THE FOLLOWING LIMITING REACTANT PROBLEMS:
17. When 16.3 g of magnesium and 4.52 g of oxygen gas react, how many grams of
magnesium oxide will be formed? Identify the limiting and excess reactants.
2 Mg + O2 → 2 MgO
18. If 25.3 g of aluminum reacts with 25.3 g of copper(II) sulfate, how many grams of
copper are formed? Identify the limiting and excess reactants in this single
replacement reaction.
2 Al + 3 CuSO4 → 3 Cu + Al2(SO4)3
19. Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 mL
of 0.250M Pb(NO3)2. How many grams of lead are formed in this single
replacement reaction?
Zn + Pb(NO3)2 → Pb + Zn(NO3)2
20. If 24.5 g of iron are placed in 1.00 L of 0.25M HCl, how many grams of FeCl2 are
obtained? Identify the limiting and excess reactants in this single replacement
reaction.
Fe + 2 HCl → FeCl2 + H2
PERFORM THE FOLLOWING PERCENT YIELD CALCULATIONS:
21. If 12.5 g of copper react with excess chlorine gas, then 25.4 g of copper(II)
chloride are produced. Find the theoretical and percent yields.
Cu + Cl2 → CuCl2
22. If 6.57 g of iron react with an excess of hydrochloric acid, HCl, then 11.2 g of
iron(II) chloride are obtained in addition to hydrogen gas. Find the theoretical
and percent yields.
Fe + 2 HCl → FeCl2 + H2
23. If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75
g of oxygen gas are also given off. Find the theoretical and percent yields.
2 KClO3 → 2 KCl + 3O2
Name
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Date
_ Class
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11-2 Practice Problems
1. Determine the mass of lithium hydroxide
produced when 0.38 g of lithium nitride
reacts with water according to the
following equation:
Li3N + 3H20 -+ NH3 + 3LiOH
7. Determine the mass of sodium nitrate
produced when 0.73 g of nickel(II) nitrate
reacts with sodium hydroxide according
to the following equation:
Ni(N03)2 + 2NaOH -+ Ni(OH)2 + 2NaN03
2. What mass of sodium chloride is
produced when chlorine reacts with
0.29 g of sodium iodide?
8. Determine the mass of calcium
hydroxide produced when calcium
carbide reacts with 0.64 g of water
according to the following equation:
CaC2 + 2H20 ---> Ca(OH)2 + C 2H 2
3. Determine the mass of carbon dioxide
produced when 0.85 g of butane reacts
with oxygen according to the following
equation:
2C4H lO + 1302 -+ 8C02 + 10H20
9. How many grams of ozone (03) must
decompose to produce 0.87 g of oxygen?
4. Determine the mass of antimony produced
when 0.46 g of antimony(III) oxide reacts
with carbon according to the following
equation:
5b20 3 + 3C ---> 25b + 3CO
10. Find the mass of sugar (C6H 120 6)
required to produce 1.82 L of carbon
dioxide gas at 5TP from the reaction
described by the following equation:
C 6H 120 6 -+ 2C2H 60 + 2C02
5. What mass of hydrogen peroxide (H 20 2)
must decompose to produce 0.77 g of
water?
11. How many liters of oxygen are necessary
for the combustion of 425 g of sulfur,
assuming that the reaction occurs at 5TP?
The balanced equation is 5 + 02 ---> 502'
6. What mass of carbon monoxide must react
with oxygen to produce 0.69 g of carbon
dioxide?
12. Find the mass of benzene (C6H 6) required
to produce 2.66 L of carbon dioxide gas at
5TP from the reaction described by the
following equation:
2C6H 6 + 1502 -+ 6H20 + 12C02
© Prentice-Hall, Inc.
Chapter 11
13
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11-2 Practice Problems (continued)
13. Find the mass of sodium required to
produce 5.68 L of hydrogen gas at STP
from the reaction described by the
following equation:
2Na + 2H 20 ---+ 2NaOH + H 2
14. How many liters of oxygen are necessary
for the combustion of 277 g of carbon
monoxide, assuming that the reaction
occurs at STP? The balanced equation is
2CO + 02 ---+ 2C02
20. What volumes of H 2S gas and oxygen are
necessary to produce 14.2 L of sulfur
dioxide gas? The balanced equation is
2H2S + 302 ---+ 2S02 + 2H20
21. What volumes of sulfur dioxide and
dihydrogen sulfide gases are necessary to
produce 11.4 L of water vapor? The
balanced equation is
S02 + 2H2S ---+ 3S + 2H20
15. How many liters of oxygen are necessary
for the combustion of 134 g of magnesium,
assuming that the reaction occurs at STP?
The balanced equation is
2Mg + 02 ---+ 2MgO
16. Find the mass of aluminum required to
produce 4.72 L of hydrogen gas at STP
from the reaction described by the
following equation:
2Al + 3H2S04 ---+ AliSO4)3 + 3H2
17. How
many liters of hydrogen are
produced if 225 g of iron reacts with
hydrochloric acid, assuming that the
reaction occurs at STP? The balanced
equation is
Fe + 2HCl ---+ FeCl2 + H 2
22. Glucose (C 6H 12 0
6 ) burns in oxygen to
produce carbon dioxide and water
vapor as described in the following
equation: C 6H 120 6 + 602 ---+ 6H20 + 6C02.
What volume of carbon dioxide is
produced when 3.7 L of oxygen are
consumed?
23. The
compound TNT (trinitrotoluene)
decomposes explosively into carbon,
carbon monoxide, hydrogen, and nitrogen.
What volumes of hydrogen and nitrogen
are produced if 5.8 L of CO is produced?
The balanced equation is
2C 7H s(N0 2)3 ---+ 2C + 12CO + 5H2 + 3N2
24. Nitroglycerin decomposes explosively to
18. Find the mass of S8 required to produce
2.47 L of sulfur dioxide gas at STP from the
reaction described by the following
equation:
produce carbon dioxide, water, nitrogen,
and oxygen. What volumes of nitrogen
and oxygen are produced if 4.3 L of carbon
dioxide is produced? The balanced
equation is
4C3H s(N03 )3 -> 12C02 + 10H20 + 02 + 6N2
19. Propane (C 3H 8) burns in oxygen to
produce carbon dioxide and water
vapor. The balanced equation for this
reaction is C3 H g + 502 ---+ 4H 20 + 3C02·
What volume of carbon dioxide is
produced when 2.8 L of oxygen are
consumed?
14
Chapter 11
25. Acetylene (C 2H 2) burns in oxygen to
produce carbon dioxide and water. The
balanced equation for this reaction is
2C2H 2 + 502 ---+ 2H20 + 4C02" What
volume of carbon dioxide is produced
when 1.6 L of oxygen are consumed?
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