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Stoichiometry Test Review

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 

Which of the following would be investigated in stoichiometry?
a.
the masses of hydrogen and oxygen in water
b.
the amount of energy released in chemical reactions
c.
the mass of potassium required to produce a known mass of potassium chloride
d.
the types of bonds that break and form when acids react with metals
 

 2. 

In the reaction N2 + 3H2 ® 2NH3, what is the mole ratio of nitrogen to ammonia?
a.
1:1
c.
1:3
b.
1:2
d.
2:3
 

 3. 

In the reaction 2Al2O3 ® 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
a.
10:6
c.
2:3
b.
3:4
d.
4:3
 

 4. 

In the equation 2KClO3 ® 2KCl + 3O2, how many moles of oxygen are produced from 3.0 mol of KClO3 ?
a.
1.0 mol
c.
3.0 mol
b.
2.5 mol
d.
4.5 mol
 

 5. 

For the reaction N2 + 3H2 ® 2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia?
a.
9.0 mol
c.
27 mol
b.
18 mol
d.
36 mol
 

 6. 

For the reaction AgNO3 + NaCl ® NaNO3 + AgCl, how many moles of silver chloride, AgCl, are produced from 7 mol of silver nitrate AgNO3?
a.
1.0 mol
c.
7.0 mol
b.
2.3 mol
d.
21 mol
 

 7. 

For the reaction 2Na + 2H2O ® 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol of water?
a.
40. g
c.
120 g
b.
80. g
d.
240 g
 

 8. 

In the reaction A + B ® C + D, if the quantity of B is insufficient to react with all of A,
a.
A is the limiting reactant.
c.
there is no limiting reactant.
b.
B is the limiting reactant.
d.
no product can be formed.
 

 9. 

To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first calculate
a.
the mass of 100 mol of A and B.
b.
the masses of all products.
c.
the bond energies of A and B.
d.
the number of moles of B and the number of moles of A available.
 

 10. 

For the reaction C + 2H2 ® CH4, how many moles of hydrogen are required to produce 10 mol of methane (CH4)?
a.
2 mol
c.
10 mol
b.
4 mol
d.
20 mol
 

 11. 

For the reaction 2H2 + O2 ® 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?
a.
2.00 g
c.
54.0 g
b.
6.00 g
d.
108 g
 

 12. 

For the reaction 2Fe + O2 ® 2FeO, how many grams of iron(II) oxide are produced from 8.00 mol of iron?
a.
71.8 g
c.
712 g
b.
574 g
d.
1310 g
 

 13. 

For the reaction Cl2 + 2KBr ® 2KCl + Br2, how many moles of potassium chloride are produced from 119 g of potassium bromide and excess chlorine?
a.
0.119 mol
c.
0.581 mol
b.
0.236 mol
d.
1.00 mol
 

 14. 

For the reaction 2KlO3 ® 2KCl + 3O2, how many moles of potassium chlorate are required to produce 250 g of oxygen?
a.
2.0 mol
c.
4.9 mol
b.
4.3 mol
d.
5.2 mol
 

 15. 

For the reaction 2Zn + O2 ® 2ZnO, how many grams of zinc oxide can be produced from 100.g of zinc and 100.g oxygen?
a.
100. g
c.
189 g
b.
124 g
d.
200. g
 

 16. 

For the reaction 2Na + 2H2O ® 2NaOH + H2, calculate the percent yield if 80. g of water react with excess sodium to produce 4.14 g of hydrogen.
a.
87%
c.
92%
b.
89%
d.
98%
 

 17. 

Which reactant controls the amount of product formed in a chemical reaction?
a.
excess reactant
c.
composition reactant
b.
mole ratio
d.
limiting reactant
 

 18. 

What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
a.
mole ratio
c.
Avogadro yield
b.
percent yield
d.
excess yield
 

 19. 

What is the measured amount of a product obtained from a chemical reaction?
a.
mole ratio
c.
theoretical yield
b.
percent yield
d.
actual yield
 

 20. 

What is the maximum possible amount of product obtained in a chemical reaction?
a.
theoretical yield
c.
mole ratio
b.
percent yield
d.
actual yield
 

 21. 

If the percent yield is equal to 100%, then
a.
the actual yield is greater than the theoretical yield.
b.
the actual yield is equal to the theoretical yield.
c.
the actual yield is less than the theoretical yield.
d.
there was no limiting reactant.
 

 22. 

Which of the following would NOT be studied in the branch of chemistry called stoichiometry?
a.
the mole ratio of aluminum and chlorine in aluminum chloride
b.
the amount of energy required to break the ionic bonds in calcium fluoride
c.
the mass of carbon produced when a known mass of sucrose decomposes
d.
the number of moles of hydrogen that react completely with a known quantity of oxygen
 

Problems
 

 23. 

How many grams of sodium hydroxide is produced if 20.0 g of sodium metal reacts with excess water according to the chemical equation 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g)?
 

 24. 

How many grams of hydrogen gas is produced if 20.0 mol of Zn are added to excess hydrochloric acid (HCl) according to the equation Zn(s) +2HCl(aq) ® ZnCl2(aq) + H2(g)?
 

 25. 

How many grams of ammonium sulfate can be produced if 30.0 mol of H2SO4 react with excess NH3 according to the equation 2NH3(aq) + H2SO4(aq) ® (NH4)2SO4(aq)?
 

 26. 

How many moles of Ag can be produced if 350. g of Cu are reacted with excess AgNO3 according to the equation Cu(s) + 2AgNO3(aq) ® 2Ag(s) + Cu(NO3)2(aq)?
 



 
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