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Chapter 9 Prep-Test Per 2

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

 1. 
What is the molar mass of ammonia (nitrogen trihydride)?
a.
15.0 g/mol
c.
43.0 g/mol
b.
17.0 g/mol
d.
45.0 g/mol
 

 2. 
For the reaction SO3 + H2O ® H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid?
a.
80.0 g
c.
240. g
b.
160. g
d.
320. g
 

 3. 
For the reaction Pb(NO3)2 + 2KI ® PbI2 + 2KNO3, how many moles of lead iodide are produced from 332. g of potassium iodide?
a.
1.00 mol
c.
3.00 mol
b.
1.50 mol
d.
10.0 mol
 

 4. 
For the reaction 2HNO3 + Mg(OH)2 ® Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced from 4.00 mol of nitric acid?
a.
148 g
c.
296 g
b.
445 g
d.
592 g
 

 5. 
The coefficients in a chemical equation represent the
a.
masses, in grams, of all reactants and products.
b.
relative numbers of moles of reactants and products.
c.
number of atoms in each compound in a reaction.
d.
number of valence electrons involved in the reaction.
 

 6. 
In the chemical reaction wA + xB ® yC + zD, a comparison of the number of moles of A to the number of moles of C would be a(n)
a.
mass ratio.
c.
electron ratio.
b.
mole ratio.
d.
energy proportion.
 

 7. 
In the reaction Zn + H2SO4 ® ZnSO4 + H2, what is the mole ratio of zinc to sulfuric acid?
a.
1:6
c.
1:2
b.
1:1
d.
3:1
 

 8. 
In the reaction C + 2H2 ® CH4, what is the mole ratio of hydrogen to methane?
a.
1:1
c.
1:2
b.
2:1
d.
2:4
 

 9. 
In the reaction N2 + 3H2 ® 2NH3, what is the mole ratio of hydrogen to ammonia?
a.
1:1
c.
3:2
b.
2:1
d.
6:8
 

 10. 
The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) ® 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?
a.
1.0 mol
c.
3.0 mol
b.
2.0 mol
d.
6.0 mol
 

 11. 
For the reaction 2Na + 2H2O ® 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 moles of water?
a.
40. g
c.
120 g
b.
80. g
d.
240 g
 

 12. 
For the reaction 2KClO3 ® 2KCl + 3O2, how many moles of potassium chlorate are required to produce 96 g of oxygen?
a.
2.0 mol
c.
4.0 mol
b.
4.5 mol
d.
5.0 mol
 

 13. 
For the reaction 2Na + Cl2 ® 2NaCl, how many grams of sodium chloride can be produced from 142. g of chlorine?
a.
117 g
c.
400 g
b.
234 g
d.
825 g
 

 14. 
For the reaction 2Zn + O2 ® 2ZnO, how many grams of zinc oxide can be produced from 196 g of zinc?
a.
100. g
c.
122 g
b.
244 g
d.
200. g
 

 15. 
For the reaction Cl2 + 2KBr ® 2KCl + Br2, calculate the percent yield if 213 g of chlorine react with excess potassium bromide to produce 432 g of bromine.
a.
70.0%
c.
90.0%
b.
100.%
d.
80.0%
 

 16. 
For the reaction CH4 + 2O2 ® 2H2O + CO2, calculate the percent yield of carbon dioxide if 1600. g of methane react with excess oxygen to produce 2200. g of carbon dioxide.
a.
50.00%
c.
100.0%
b.
80.00%
d.
90.00%
 

 17. 
In the reaction 2CO(g) + Omc017-1.jpg(g) ® 2COmc017-2.jpg(g), what is the ratio of moles of oxygen used to moles of COmc017-3.jpg produced?
a.
1:1
c.
1:2
b.
2:1
d.
2:2
 

 18. 
How many moles of aluminum are needed to react completely with 1.5 mol of FeO?
2Al(s) + 3FeO(s) ® 3Fe(s) + Almc018-1.jpgOmc018-2.jpg(s)
a.
1.5 mol
c.
3.0 mol
b.
1.0 mol
d.
0.5 mol
 

 19. 
Calculate the number of moles of Almc019-1.jpgOmc019-2.jpg that are produced when 0.60 mol of Fe is produced in the following reaction.
2Al(s) + 3FeO(s) mc019-3.jpg 3Fe(s) + Almc019-4.jpgOmc019-5.jpg(s)
a.
0.20 mol
c.
0.60 mol
b.
0.40 mol
d.
0.90 mol
 

 20. 
Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Femc020-1.jpgOmc020-2.jpg are formed when 27.9 g of Fe reacts completely with oxygen?
mc020-3.jpg
a.
12.0 g
c.
30.0 g
b.
40.0 g
d.
95.0 g
 

 21. 
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
 

 22. 
If you start with 10.0 moles of C3H8 (propane) and 10.0 moles of O2, what is the limiting reactant.
C3H8(g) + 5O2(g) ®  3CO2(g) + 4H2O(g) 
a.
oxygen
c.
carbon dioxide
b.
propane
d.
water
 

Matching
 
 
Match each item with the correct statement below.
a.
actual yield
e.
limiting reagent
b.
percent yield
f.
mass
c.
theoretical yield
g.
number of molecules
d.
excess reagent
h.
volume
 

 23. 

 This quantity can always be used in the same way as moles when interpreting balanced chemical equations.
 

 24. 

 This is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products.
 

 25. 

 This is conserved in every ordinary chemical reaction.
 

 26. 

 the reactant that determines the amount of product that can be formed in a reaction
 

 27. 

 the maximum amount of product that could be formed from given amounts of reactants
 

 28. 

 the reactant that is not completely used up in a reaction
 

 29. 

 the amount of product formed when a reaction is carried out in the laboratory
 

 30. 

 the ratio of the actual yield to the theoretical yield
 



 
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