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Chapter 9 Prep-Test

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

 1. 
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
 

 2. 
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
 

 3. 
How many moles of Almc003-1.jpgOmc003-2.jpgare produced when 0.60 mol of Fe is made in the following reaction.                 2Al(s) + 3FeO(s) mc003-3.jpg 3Fe(s) + Almc003-4.jpgOmc003-5.jpg(s)
a.
0.20 mol
c.
0.60 mol
b.
0.40 mol
d.
0.90 mol
 

 4. 
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
 

 5. 
In the reaction N2 + 3H2 ® 2NH3, what is the mole ratio of hydrogen to NH3?
a.
1:1
c.
3:2
b.
2:1
d.
6:8
 

 6. 
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%
 

 7. 
For the reaction Cl2 + 2KBr ® 2KCl + Br2, calculate the percent yield if 213 g of chlorine reacts with excess potassium bromide to produce 432 g of bromine.
a.
70.0%
c.
90.0%
b.
100.%
d.
80.0%
 

 8. 
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
 

 9. 
How many moles of aluminum are needed to react completely with 1.5 mol of FeO?
2Al(s) + 3FeO(s) ® 3Fe(s) + Almc009-1.jpgOmc009-2.jpg(s)
a.
1.5 mol
c.
3.0 mol
b.
1.0 mol
d.
0.5 mol
 

 10. 
Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Femc010-1.jpgOmc010-2.jpg are formed when 27.9 g of Fe reacts completely with oxygen?
mc010-3.jpg
a.
12.0 g
c.
30.0 g
b.
40.0 g
d.
95.0 g
 

 11. 
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
 

 12. 
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
 

 13. 
In the reaction 2CO(g) + Omc013-1.jpg(g) ® 2COmc013-2.jpg(g), what is the ratio of moles of oxygen used to moles of COmc013-3.jpg produced?
a.
1:1
c.
1:2
b.
2:1
d.
2:2
 

 14. 
The Haber process for producing ammonia (NH3) 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
 

 15. 
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
 

 16. 
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
 

 17. 
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.
 

 18. 
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.
 

 19. 
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
 

 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. 
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
 

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

 22. 

 the reactant that is not completely used up in a reaction
 

 23. 

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

 24. 

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

 25. 

 This is conserved in every ordinary chemical reaction.
 

 26. 

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

 27. 

 the ratio of the actual yield to the theoretical yield
 



 
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