Chemistry Chapter 12A (Prentice)
 
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Chemistry Chapter 12A (Prentice)

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
 

 1. 

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

 2. 

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.
 

 3. 

This is conserved in every ordinary chemical reaction.
 

 4. 

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

 5. 

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

 6. 

the reactant that is not completely used up in a reaction
 

 7. 

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

 8. 

the ratio of the actual yield to the theoretical yield
 

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

 9. 

The calculation of quantities in chemical equations is called ____.
a.
stoichiometry
c.
percent composition
b.
dimensional analysis
d.
percent yield
 

 10. 

If 1 egg and 1/3 cup of oil are needed for each bag of brownie mix, how many bags of brownie mix do you need if you want to use up all 3 eggs and 1 cup of oil?
a.
1
c.
3
b.
2
d.
4
 

 11. 

What is conserved in the reaction shown below?
Hmc011-1.jpg(g) + Clmc011-2.jpg(g) ® 2HCl(g)
a.
mass only
c.
mass, moles, and molecules only
b.
mass and moles only
d.
mass, moles, molecules, and volume
 

 12. 

What is conserved in the reaction shown below?
Nmc012-1.jpg(g) + 3Fmc012-2.jpg(g) ® 2NFmc012-3.jpg(g)
a.
atoms only
c.
mass and atoms only
b.
mass only
d.
moles only
 

 13. 

In every chemical reaction, ____.
a.
mass and molecules are conserved
c.
mass and atoms are conserved
b.
moles and liters are conserved
d.
moles and molecules are conserved
 

 14. 

In a chemical reaction, the mass of the products ____.
a.
is less than the mass of the reactants
b.
is greater than the mass of the reactants
c.
is equal to the mass of the reactants
d.
has no relationship to the mass of the reactants
 

 15. 

In any chemical reaction, the quantities that are preserved are ____.
a.
the number of moles and the volumes
b.
the number of molecules and the volumes
c.
mass and number of atoms
d.
mass and moles
 

 16. 

The first step in most stoichiometry problems is to ____.
a.
add the coefficients of the reagents
c.
convert given quantities to volumes
b.
convert given quantities to moles
d.
convert given quantities to masses
 

 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. 

Which of the following is true about the total number of reactants and the total number of products in the reaction shown below?
Cmc018-1.jpgHmc018-2.jpg(l) + 8Omc018-3.jpg(g) ® 5COmc018-4.jpg(g) + 6Hmc018-5.jpgO(g)
a.
9 moles of reactants chemically change into 11 moles of product.
b.
9 grams of reactants chemically change into 11 grams of product.
c.
9 liters of reactants chemically change into 11 liters of product.
d.
9 atoms of reactants chemically change into 11 atoms of product.
 

 19. 

Which of the following is an INCORRECT interpretation of the balanced equation shown below?
2S(s) + 3Omc019-1.jpg(g) ® 2SOmc019-2.jpg(g)
a.
2 atoms S + 3 molecules Omc019-3.jpg ® 2 molecules SOmc019-4.jpg
b.
2 g S + 3 g Omc019-5.jpg ® 2 g SOmc019-6.jpg
c.
2 mol S + 3 mol Omc019-7.jpg ® 2 mol SOmc019-8.jpg
d.
none of the above
 

 20. 

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s) ® 3Fe(s) + Almc020-1.jpgOmc020-2.jpg(s)
a.
1.2 mol
c.
1.6 mol
b.
0.8 mol
d.
2.4 mol
 

 21. 

Calculate the number of moles of Almc021-1.jpgOmc021-2.jpg that are produced when 0.60 mol of Fe is produced in the following reaction.
2Al(s) + 3FeO(s) mc021-3.jpg 3Fe(s) + Almc021-4.jpgOmc021-5.jpg(s)
a.
0.20 mol
c.
0.60 mol
b.
0.40 mol
d.
0.90 mol
 

 22. 

How many moles of glucose, Cmc022-1.jpgHmc022-2.jpgOmc022-3.jpg, can be "burned" biologically when 10.0 mol of oxygen is available?
Cmc022-4.jpgHmc022-5.jpgOmc022-6.jpg(s) + 6Omc022-7.jpg(g) ® 6COmc022-8.jpg(g) + 6Hmc022-9.jpgO(l)
a.
0.938 mol
c.
53.3 mol
b.
1.67 mol
d.
60.0 mol
 

 23. 

Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum?
2Al(s) + 3Hmc023-1.jpgSOmc023-2.jpg(aq) ® Almc023-3.jpg(SOmc023-4.jpg)mc023-5.jpg(aq) + 3Hmc023-6.jpg(g)
a.
0.100 mol
c.
15.0 mol
b.
10.0 mol
d.
22.5 mol
 

 24. 

When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction?
4Fe(s) + 3Omc024-1.jpg(g) ® 2Fe2Omc024-2.jpg(s)
a.
1.2 mol
c.
2.4 mol
b.
1.8 mol
d.
3.2 mol
 

 25. 

At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water?
2Hmc025-1.jpg(g) + Omc025-2.jpg(g) ® 2Hmc025-3.jpgO(g)
a.
1.8 L
c.
2.0 L
b.
3.6 L
d.
2.4 L
 

 26. 

Which type of stoichiometric calculation does not require the use of the molar mass?
a.
mass-mass problems
c.
mass-particle problems
b.
mass-volume problems
d.
volume-volume problems
 

 27. 

The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NOmc027-1.jpg is formed?
mc027-2.jpg
a.
1.00 g
c.
2.88 g
b.
2.00 g
d.
32.0 g
 

 28. 

Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Femc028-1.jpgOmc028-2.jpg are formed when 16.7 g of Fe reacts completely with oxygen?
mc028-3.jpg
a.
12.0 g
c.
47.8 g
b.
23.9 g
d.
95.6 g
 

 29. 

When glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of Cmc029-1.jpgHmc029-2.jpgOmc029-3.jpg completely reacted with oxygen?
a.
1.5 g
c.
11 g
b.
1.8 g
d.
66 g
 

 30. 

Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate would be formed if 250 g Hmc030-1.jpgSOmc030-2.jpg completely reacted with aluminum?
mc030-3.jpg
a.
0.85 g
c.
450 g
b.
290 g
d.
870 g
 



 
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