Chemistry Reference
In-Depth Information
10.22
Calculate the number of moles of
Ba(OH)
2
that will
(c) Calculate the number of moles of butane required
to produce that number of moles of carbon dioxide.
(d) Calculate the mass of butane in that number of
moles.
(e) Combine the calculations for parts (b)-(d) into one
factor label solution.
react with 0.600 mol of
H
3
PO
4
to form
Ba(H
2
PO
4
)
2
.
10.23
Which of the following samples of metal can produce
the most hydrogen by reaction with HCl?
0.500 mol Zn
0.500 mol Al
0.500 mol Mg
10.24
How many moles of
C
6
H
14
can be produced by the re-
10.34
(a) In an internal combustion engine, octane,
burns in limited oxygen supply to produce carbon
monoxide and water. Write a balanced equation for
the reaction.
(b) Calculate the number of moles of carbon monoxide
in 75.7 g of carbon monoxide.
(c) Calculate the number of moles of octane required to
produce that number of moles of carbon monoxide.
(d) Calculate the mass of octane in that number of moles.
(e) Combine the calculations for parts (b)-(d) into one
factor label solution.
C
8
H
18
,
action of 4.86 mol of
H
2
and sufficient
C
6
H
10
?
The bal-
anced equation is
C
6
H
10
(
/
)
2 H
2
(g) £ C
6
H
14
(
/
)
10.25
How many moles of oxygen gas are required for the
combustion of 7.04 mol of octane,
C
8
H
18
,
to yield
CO
2
and water?
10.26
How many moles of oxygen gas are required for the in-
complete combustion of 7.80 mol of octane,
yielding CO and
C
8
H
18
,
H
2
O?
10.27
How many moles of oxygen gas are required for the
complete combustion of 6.16 mol of butane,
C
4
H
10
?
10.35
Calculate the mass of each of the following that is nec-
essary to produce 4.00 mol of AgCl by reaction with
(Compare with Problem 10.9.)
10.28
How many moles of
AlCl
3
are also produced along with
2.46 mol of
H
2
O
from the reaction of
Al(OH)
3
and HCl?
AgC
2
H
3
O
2
.
(a)
CoCl
3
(b)
CaCl
2
(c) KCl
10.29
How many moles of
MgCl
2
are produced along with
0.750 mol of
CO
2
from the reaction of
Mg(HCO
3
)
2
and
10.36
Calculate the mass of each of the following reagents
that is necessary to produce 1.75 mol of AgCl by reac-
tion with
(a)
HCl?
AgNO
3
.
2
10.30
(a) Calculate the number of millimoles of
CrO
that
4
Co
2
reacts with 7.00 mmol of
according to the
PtCl
2
(b)
SrCl
2
(c)
NiCl
2
following equation:
10.37
Calculate the mass of product produced by each of the
following combinations:
(a) 15.0 g of sodium with excess bromine
(b) 25.0 g of magnesium with excess oxygen
(c) 35.0 g of aluminum with excess sulfur
3 Co
2
(aq)
CrO
2
(aq)
8 H
(aq) £
4
3 Co
3
(aq)
Cr
3
(aq)
4 H
2
O(
/
)
(b) How many millimoles of water are produced?
10.31
Part of an 8.00-mmol sample of HgO was decomposed
by heating, and 1.50 mmol of was produced.
(a) Write the balanced equation for the reaction.
(b) Which of the numbers of millimoles given in the
problem is governed by the balanced equation?
(c) Calculate the percentage of HgO that decomposed.
O
2
10.38
Excess
AgNO
3
(aq)
was added to a sample of
and 12.1 g of AgCl(s) was produced. What
FeCl
3
(aq),
mass of
FeCl
3
was present initially?
10.39
Aluminum is produced commercially by high-
temperature electrolysis of aluminum oxide dissolved
in a nonaqueous melt. The electrodes are carbon.
10.2 Mass Calculations for Chemical Reactions
Al
2
O
3
(solution)
3 C(s) £ 2 Al(
/
)
3 CO(g)
10.32
Calculate the number of moles of that are produced
by the reaction of aqueous HCl with 2.48 g of metallic
(a) Zn.
(b) Cd.
(c) Explain why the numbers of moles of produced
in parts (a) and (b) differ greatly, even though the
same number of grams of metal is used in each
case.
H
2
Calculate the mass of
Al
2
O
3
used to produce 10.0 met-
(10.0
10
6
g)
ric tons
of aluminum by this process.
10.40
Caution:
The following reactions can proceed explo-
sively! Calculate the number of moles of hydrogen that
can be produced by reaction with water of (a) 0.600 g
of lithium and (b) 0.600 g of barium. (c) Explain the
difference.
H
2
10.41
Silver can be prepared from aqueous silver nitrate by
reaction with zinc metal. Zinc nitrate is formed.
(a) Write a balanced equation for the reaction.
(b) Calculate the number of moles of zinc in 12.10 g of
zinc.
10.33
(a) Butane, burns in excess oxygen to produce
carbon dioxide and water. Write a balanced equa-
tion for the reaction.
(b) Calculate the number of moles of carbon dioxide in
14.9 g of carbon dioxide.
C
4
H
10
,
