S
Name:
Student#
_______________
Chapter 9 Review
PART I Circle the letter of the term or phrase that best completes each statement or best
answers each questions.
1.
A
2.
‘
3.
j
4.
h
A balanced chemical equation allows one to determine the
~
mole ratio of any two substances in the reaction.
b.
energy released in the reaction.
c.
electron configuration of all elements in the reaction.
d.
mechanism involved in the reaction.
The coefficients in a chemical equation represent the
a.
masses, in grams, of all reactants and products.
fl 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.
Actual yield must be determined by
experiments.
b.
calculations.
c.
theoretical yield.
d.
estimation.
C
To determine the limiting reactant in a chemical reaction involving known masses
of the two reactants, which of the following would be most useful?
a.
determining the masses of 100 mol of each reactant
b.
determining the molar masses of the products
c.
calculating bond energies
•
calculating the mass of a single product formed from each reactant
s. _____Which expression can be used to solve a mass-to-mole conversion for the
equation 2HCI -*H2 + Cl2?
a.
b.
c.
d.
JVt44. t,n.ck
massHClx
I mol HC1
I mol Cl2
x
molarmass HCI 2 molHCl
lmolCl2
xmassHCi
2 molHCl
2molHCl
imolilCi
x
xmassJ4Cl
1 mol Cl2 molar mass HC1
lmoICl2
massHClx molarmassHClx
2 mol HCI
9
Name: ____________________________________________Studerit#
6.
In the equation 2AbO3
oxygen?
a. 10:6
b. 3:4
c. 2:3
—,
_______________
4A1 + 302, what is the mole ratio of aluminum to
a :3
7.
Fewer steps are required to solve stoichiometry problems when
a.the reactant is given in grams and the product is sought in grams.
reactant is given in moles and the product is sought in moles.
c.the reactant is given in grams and the product is sought in liters.
d.the reactant is given in liters and the product is sought in number of atoms.
-
8.
Which of the following mathematical expressions correctly states the relationship
among percentage yield, actual yield, and theoretical yield?
percentage yield
xlOO
theoretical yield
actual yield
b. percentage yield =
x 100
theoretical yield
actual yield
c. theoretical yield =
x 100
percentage yield
a. actual yield
=
.
®Both (b) and (c)
9.
The participation of reactants in a chemical reaction is restricted by the
limiting reactant.
b. limiting product.
c. excess reactant.
d. excess product.
®
10. ______Which of the following expressions is not a legitimate conversion factor?
1 mol
a.
6.022xl&’ atoms
b. 28.02gN2
lmolN2
a
lgC
6.022x 1023 atomsC
d. 2.02gH2
lmolH2
C4tek91teY~L.4.
Name: ____________________________________________Student#
ii.
‘3
12.
13.
_______________
The limiting reactant of a reaction can be used to calculate the
a. actual yield.
theoretical yield.
c. experimental yield.
d. Both (a) and (c)
If the percentage yield for a chemical reaction is 80.0%, the
actual yield is 80.0 g for every theoretical yield of 100. g.
theoretical yield is 80.0 g for every actual yield of 100. g.
c. actual yield is 80 times as much as the theoretical yield.
d. theoretical yield is 80 times as much as the actual yield.
A
In the reaction represented by the equation A + B .—* C + D, if there is more
reactant B than is required to completely react with all of A, then
O A is the limiting reactant.
B is the limiting reactant.
c. there is no limiting reactant.
d. no product can be fonned.
14. ______If a chemist calculates the maximum amount of product that could be obtained in
a chemical reaction, he or she is calculating the
C~ theoretical yield.
b. percentage yield.
c. mole ratio.
d. actual yield.
PART II Write the correct equation or term in the space provided.
15.Fill in the steps required to find the number of grams of substance B produced from the
number of grams of substance A.
gramsofA->
jjO4
4
___________-,gramsofB
16. The conversion factor for deriving the number of moles of salicylic acid, C7H603, from a
given number of grams of salicylic acid is
17. The substance that restricts the amount of other reactants used in a chemical reaction is
known as the
tja...
S_i1..~
i.
18. The measured amount of product obtained from a chemical reaction is called the
fAA
_
I
.M44. tank
C$CLa~~L4t4y1
C4te*Stc.tte&..
Name: ____________________________________________Student#
_______________
19. The substance that is not completely used up in a chemical reaction is known as the
A
*A
h’.....~t1Aa
20. If the theoretical yield for a chemical reaction is
theactualyieldis
-
100. g and the percentage yield is 70.0%,
.
— _____
6
PART ifi Write the answers to the questions on the line to the left, and show your work
in the space provided
575
s
21. For the reaction represented by the equation
2Fe +02 2FeO, how many grams of iron oxide will be
produced from 8.00 mol of iron when 02 is in excess?
—,
8vioLJ~e-x~FØ.
~
-
°
22. If cyclohexanol is burned as a fuel according to the following
equation, how many moles of oxygen are needed to produce
13.7 mol of carbon dioxide? 2C6H120 + 1702 —* 12C02 ÷
121t0
~ ~c~E3:)
i3.7~to&c2ç
23. For the reaction represented by the equation Pb(N03)2 + 21(1
Pb12 + 21CN03, how many moles of lead iodide are
produced from 300. g of potassium iodide when Pb(N03)2 is
in excess?
K~ 3~~O
—,
~ ~
.~OYn~fPbJj
~°°~
“I40~
U
£10
llQO.@At~LX
3
S2PO~
24. For the reaction represented by the equation 2KC103 -÷ 2KCI
+ 302, how many grams of potassium chlorate are required to
produce 160.gofoxygen?
-~-~—
x
3n4~&UL
CI 3S4
O31i~L
Student #
Name:
a.oI
CÁO
25. According to the equation C3Hg + 502 —÷ 3C02 + 4H20, when
02 is in excess, how many grams of carbon dioxide are
produced from the combustion of 250. g of ethane, C3H8? C3Qll.La\~
cv,o~C3~-l~
Zc~jC34
)C
~
C~t
L~Mla~.L Cj~.4e
MOlt
]c{~
Cb~
i1 fO~
26. In the reaction represented by the equation
2Na ÷ 2H20 -+ 2NaOH + 142, how many grams of hydrogen
are produced if 120. g of Na and 80.0 g of H20 are available?
h~
\~J~t~
fllA$s
~
~b’O~2
Li
~ni&.tW≥D~ fl4b-&~
27. Calculate the percentage yield for the reaction represented by
the equation
CR4 + 202 -. 21420 + CO2 when 1000. g of CR4 react with
excess 02 to produce 2300. g of CO2.
_____________
0
.g_7
t’c~
(o~T
-
t!I1
23tO~
—
1000
jAn
4;’
Use the equation CI
+
2KBr — 2KC1
81) Th 6k h≤’C I
I,
cqq
+
~
(‘C~
Br2 for problems 28—30.
28. How many moles of potassium chloride are produced from
119 g of potassium bromide when CJ2 is in excess?
~
II ~ Kôr
Ci
3Ob~ CL
3co~
k~
.at t..~
29. How many grams of potassium chloride can be produced from
300. g each of Cl2 and KBr?
7OMO~
x
8 4~et.Kcj
MOLt ~‘LI
lmett QJ).
S*t*.t&r~
dsrhM&LLI
ji%(3’~
~~flI~L~Kc
C~
L
51. Me&gu~~
7
1~4
2~’~~jxc a
CL.j~tg 9
KU
Name: __________________________________________________Student It
0.9
~c
.
/p
~
P~
~pL
(v~&4C/L.
~c9.$t
•
fl
Determine the molarity of a solution prepared by dissolving
1~ 1.6 gof citric acid, C
• (COOH, in water and then diluting the
resulting solution to 35’’.O fliL.
~737O 4’]c’
-
)Lfl
30. What is the percentage yield if 200. g of Cl2 react with an
excess of KBr to produ ~ Bra? &-l-uo~~ ~icI~
)c
~oo>CI~
_________________
sULC~3x
I
-
‘ci 1~
i37O~~~I
3.50EC
-
A.
32. What is’ e molarity of a salt solution made by dissolving
280.0 mg of NaC1 in 2.00 mL of water?
~ 79fy/OJ~~f
A
iO~m~
n&~L
q7q(~(Q?~0)j~Q
L/qy
a.gq~mAiac1
M
C.OU 33. What is the molarity of a solution that contains 39’.’ go
acetic acid, CH3COOH, dissolved in enough acetone to make 1000.0 mL of
solution?
390.0
e~Je
C143C004.I y’
1DO.O(O~~
~
asP
IL
~ (
1Jr~~ 6/z~
J6&tta,.ek
C$’CLn.(4t411
e~~J3cco