'-.-_______
Class:
Date:
_
ID: B
_.stry: Chapter 12: Stoichiometry
/
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
1. Which of the following is true about the total number of reactants and the total number of products in the
reaction shown below?
CSH12(l) + 8°2 (g) ~ 5C02(g) + 6H20(g)
a.
b.
c.
d.
9 grams of reactants chemically change into 11 grams of product.
9 liters of reactants chemically change into 11 liters of product.
9 atoms of reactants chemically change into 11 atoms of product.
9 moles of reactants chemically change into 11 moles of product.
2. Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams ofFe203
J2
)Cf-ife}
when 16.7 g of Fe reacts completely with oxygen?
4Fe(s) + 3°2 (g) ~ 2Fe203(s)
a. 12.0 g
(C).
b. 95.6 g
'-t.
3. What is conserved in the reaction shown below?
N2(g)+3F2(g)~2NF3(g)
J
0 l..:;'
.".....
J
23.9 g
47.8 g
IAIl LW,r
V'Iln'.)':>
I~ ,'1. 4 Fe ~ _Q ;;to~~O~
).t.f-
J
z: 3.3;0,
re
'-I ~
f
f)
/tf'J.
are formed
L),...~-\.Aj] ..(
rfIUYj'(-
a. mass only
c. moles only
b. atoms only
mass and atoms only
4. Which ofthe following is an INCORRECT interpretation of the balanced equation shown below?
2S(8) + 3°2 (g) ~ 2S03(g)
@
A
a.
2gS+3g02~2gS03
b.
2 atoms S + 3 molecules 02 --+ 2 molecules S03
c.
2 mol S + 3 mol 02 -» 2 mol S03
d.
none of the above
5. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are
needed to cOl!Wletely react with 15.0 mol of aluminum?
2[I(s) + 3H2S04(aq) ~ A1iS04)3(aq) + 3H2(g)
<V
b.
22.5 mol
10.0 mol
c.
d.
X V\lUJk. U)/ ~(J.'f .:: 15 Mil'.
0.100 mol
15.0 mol
_
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/) 1
eX c( I
6. How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(tl + 3FeO(s) --+ 3Fe(s) + Al2 03 (s)
'/. rYlO!
J M i)
+ I;::: ,.
a.
b.
0.8 mol
2.4 mol
c.
d.
1.2 mol
1.6mol
(
AI
.
§"
1e. ()
.,5 ·fJw f 1£s.'t2 .
'I
y -
:; SUI; fA
~
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3
Mbf
7. At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form
water?
~2(g) + °2 (g) --+ 2H20(g)
c. 2.4 L
a. 3.6L
b. 1.8L
d. 2.0L
3·lf L
\+ ~
(c B L
f
...~
J-. Y
~ 0,,-
l-/ y. ~ L \-l ~
1
WLO(
I
A-(
R-O
Name:
--B.
ID: B
--------------------8. How many grams ofH3P04
are produced when 10.0 moles of water react with an excess OfP4010?
P40JO(s)+6H20(l)~4H3P04(aq)
a.
b.
~
'tj"3YOq.::.-
6.7 g
653 g
c.
d.
IO'~Uks"Jo
147 g
1.22 g
4.
.:
fJ~..:J
/2CZ)""y U-offJtf
y
er
1\'i
~ c:
Me.e ~
U ¥ r)
9. Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of
aluminum sulfate would be formed if250 g H2S04 comp~etrIy reacted with aluminum?
2AI(s) +3H2SO/aq)
a. 0.85 g
b. 450 g
~
+ 3H2(g)
~ AI2(S04)3(aq)
---------
c.
d.
X~ ~
OLf)3
8io g
= 0t5D, \h.r~() tf -t
_
290 g
£6
tl..J
;"'004-£
_ +-), '-}
(),.tf
1
if
tj H2'J~
0
-
I
10. The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when
11.5 gN02
is formed?
2Pb(N03)2(S)
.-1)
a. 2.88 g
c.
b. 32.0 g
d.
11. What is conserved in the reaction shown below?
H2(g) + CI2(g) ~ 2HCI(g)
a.
~.
'I. 1 o~ = !l~"
j l\Jo';(
~ 2PbO(s)+4N02(g)+02(g)
mass only
mass and moles only
c.
d.
/'
~fD.-
/gLj
__ .
1\!(}2
-
c1
()O~
1.00 g
2.00 g
mass, moles, molecules, and volume
mass, moles, and molecules only
12
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A
-fr'
Which of the following is NOT true about limiting and excess reagents?
a. The amount of product obtained is determined by the limiting reagent.
b. A balanced equation is necessary to determine which reactant is the limiting reagent.
c. The reactant that has the smallest given mass is the limiting reagent.
d. Some of the excess reagent is left over after the reaction is complete.
13. The first step in most stoichiometry problems is to __ .
a. convert given quantities to moles
c. convert given quantities to masses
b. convert given quantities to volumes
d. add the coefficients of the reagents
14. How many moles ofH3P04
are produced when 71.0 g P40lO
IP4010(S)+6H20(l)~4H~04(aq)
XIY1.0k~
L;mok.J113rU(,r
tlt'Lf
PO
a. 1.00 mol
c. 4.00 mol
0.
L(
b. 0.063 5 mol
d. 16.0 mol/I
Jl&tr~
5. In a chemical reaction, the mass of the products __ .
a. has no relationship to the mass of the reactants
b. is equal to the mass of the reactants
c. is greater than the mass of the reactants
d. is less than the mass of the reactants
Q§) Metallic copper is formed when aluminum reacts with copper(ll) sulfate. How many grams of metallic
copper can be obtained when 54.0 g of Al react with 319 g of CuS04 ?
oo
h]
A
II D
reacts completely to form H3P04?
J.f3POLf - 1--lljPOlfY
Al + 3CuS04
a. 21.2 g
b. 127 g
~
AI2(S04)3 + 3Cu
c.
d.
2
381 g
162 g
C0;
J
Name:
A
ID: B
------------------17. Glucose, C 6 H 12
°
6'
is a good source of food energy. When it reacts with oxygen, carbon dioxide and water
are formed. How many liters of CO2 are produced when] 26 g of glucose completely react with oxygen?
C6HI20JS)
a.
b.
+ 602(g) ~ 6~2(g)
+ 6I¥(l)
94.1 L
15.7 L
J LClJ
+ 673 kcal
c.
d.
5.33 L
4.21 L
:::12~ Cr, f/(J...Cftx
J
_
-
11·1.
134 '-/L
/gtJt, err
J
1-
CtJr
H,),a
18. How many liters of hydrogen gas are needed to react with CS2 to ~roduce 2.50 L of CH4 at STP?
4H2(g)+CS2(l)~
B
a.
b.
CH4(g) + 2H2S(g)
2.50 L
5.00L
c.
d.
,
10.0 L
7.S0L
L elf£{)( -.!:Li"~L II:;
:;"'/2. 1- L vII u
IO,r) L
-
19. How many grams of chromium are needed to react with an excess ofCuS04
2Cr(s) + 3CuS04(aq)
a.
b.
20.
A
X LflJ ~ ).,!JD
.21.
~ Cr2(S04)3(aq)
33.2 g
14.7 g
c.
d.
X er:8.0 g
81.5 g
o.:fti) JCf1
IL/
to produce 27.0 g Cu?
X
'1-a
J
-.
~...F(
/9 q
t1
When 0.1 mol of calcium reacts with 880 g of water, 2.24 L of hydrogen gas form ~t STP). How would the
amount of hydrogen produced change ifthe volume of water was decrease
0 40 mL (440 g)?
a. The volume of hydrogen produced would double.
~ J?-Ib StrWl1..,
;47~-P
b. No hydrogen would be produced.
/
c. Only one half the volume of hydrogen would be produced .
.f!. The volume of hydrogen produced would be the same.
How many liters of chlorine gas can be produced when 0.98 L ofHCI react with excess 02 at STP?
XL CJJ:::.
4HCI(g)+02(g)~2C12(g)+2H20(g)
a.
b.
22.
+ 3Cu(s)
7
0.49 L
3.9L
c.
d.
t
1~L He!
0.98 L
2.0L
_
-
'1'-1. <?~/y
X
'I
Of, a I.-
8~ , t L II t!
9
/
Howmany liters ofNH3, at STP, will react with 5.3 g 02 to form N02 and water? t?
1.11L
6
4NH3 (g) + 702 (g) ~ 4N02 + 6Hz O(g)
L /II ItJ :::: S' ~ OJ (}:2 y
, ~ !:- (V"3
atfuJ(}1a. 3.03 L
c. 0.00423 L
b. 6.49 L
d. 2.12 L
~ /
t:
X
.2
l:Z
23. How many liters ofNH3 are needed to react completely with 30.0 L of NO (at STP)7 a
"Id
4NH3(g) + 6N0(g) ~ 5N2(g) + 6H20(g)
L H!) :: ~O .PL if(j X
6J ~~ L IV, :3
X N
a.
b.
24.
7.5 L
5.0 L
c.
d.
120.0 L
20.0 L
=- r:Zo
/39< 'I 1. NO
I ()
L
Which type of stoichiometric calculation does not require the use of the molar mass?
a. volume-volume problems
c. mass-mass problems
b. mass-particle problems
d. mass-volume problems
-
25. In the reaction 2CO(g) + 02(g)
.
produced?
a. '2:2
b. 1:1
-7
2C02 (g), what is the ratio of moles of oxygen used to moles of CO2
~
"-
c.
d.
3
2:1
1:2