Chemistry Reference
In-Depth Information
18.3
Explain why the concentration ratios in addition to mole
ratios are governed by the balanced chemical equation
for an equilibrium system in a solution.
18.8
Write an equilibrium constant expression for each of the
following reactions:
(a)
(b)
N
2
(g)
3 H
2
(g) E 2 NH
3
(g)
18.4
(a) What is the rate of decomposition of ammonia at the
point where hydrogen and nitrogen are first intro-
duced into an empty reaction vessel at
N
2
(g)
3 H
2
(g) E 2 NH
3
(g)
heat
18.9
What is the relationship between the equilibrium con-
stant values for the two equations in each of the follow-
ing sets?
(a)
500°C
?
(b) What happens to this rate as time passes?
18.5
Write an equilibrium constant expression for the follow-
ing reaction:
N
2
O
4
(
/
) E 2 NO
2
(g)
2 NO
2
(g) E N
2
O
4
(
/
)
CH
3
OH(
/
)
HCHO
2
(
/
) E CH
3
OCHO(
/
)
H
2
O(
/
)
(b)
2 CO(g)
O
2
(g) E 2 CO
2
(g)
18.6
Write an equilibrium constant expression for each of the
following reactions:
(a)
(b)
(c)
1
2
O
2
(g) E CO
2
(g)
CO(g)
18.10
Write an equilibrium constant expression for each of the
following reactions:
(a)
(b)
(c) 2 NaHCO
3
(s) E Na
2
CO
3
(s)
H
2
(g)
I
2
(g) E HI(g)
HI(g)
H
2
(g)
I
2
(g) E 2 HI(g)
S(s)
O
2
(g) E SO
2
(g)
H
2
(g)
I
2
(s) E 2 HI(g)
2 C(s)
O
2
(g) E 2 CO(g)
18.7
Write an equilibrium constant expression for each of the
following reactions:
(a)
(b) Heat
CO
2
(g)
H
2
(g) E CO(g)
H
2
O(g)
CO
2
(g)
CO
2
(g)
H
2
(g) E CO(g)
H
2
O(g)
H
2
O(g)
Problems
18.1 Rates of Reaction
(c) How much will the surface area be if the cube is cut
nine times in each direction—vertically front to
back, vertically side to side, and horizontally (to
make 20 surfaces in each direction)?
18.11
Calculate the number of moles per liter of a gas at
and (a) 0.800 atm pressure and (b) 2.00 atm pressure.
(c) Show that, all other conditions remaining the same,
the pressure of a gas and its concentration in moles per
liter are directly proportional.
18.12
How can scouts on a camping trip get a log to burn faster?
18.13
A certain industrial process produces 10.5 mol/L of
product per minute at How could that same reac-
tion be speeded up to produce 21.0 mol/L of product per
minute without changing the nature or concentrations of
the reactants or the temperature?
18.14 A certain reaction produces 1.50 mol/L of product per
minute at How could that same reaction be
speeded up to produce 6.00 mol/L of product per minute
without change in the contents of the reaction vessel?
18.15
(a) At which of the following temperatures will the de-
composition reaction of the Haber process go fastest?
25°C
18.2 The Condition of Equilibrium
18.17
(a) At a certain point in a reaction leading to the equi-
librium system
25°C.
2 CO(g)
O
2
(g) E 2 CO
2
(g)
the rate of decomposition of is
What is the rate of combination of CO
with if this point is at the start of this experiment?
(b) What is the rate of combination of CO with
CO
2
2.28
10
5
mol/L
#
s.
O
2
O
2
if at
25°C.
this point the system is at equilibrium?
18.18
At a certain point in a reaction leading to the equilibrium
system
2 CO(g)
O
2
(g) E 2 CO
2
(g)
0°C
200°C
500°C
the rate of combination of with CO is
What is the rate of combination of CO at
O
2
6.14
10
5
mol/L
#
s.
(b) At which of these temperatures will the combination
reaction go fastest?
18.16
(a) Calculate the surface area of a cube that is 1.00 cm
on each edge (see Figure 18.1).
(b) How much will the surface area increase if the cube
is cut in half, as shown in the figure?
this point?
18.19 At a certain point in a reaction leading to the equilibrium
system
2 CO(g)
O
2
(g) E 2 CO
2
(g)
