1.( D
) For the reaction system N2(g) + 3H2(g)
2NH3(g) at equilibrium, ∆H is –92 kJ. In order to
both shift the equilibrium and increase the yield of ammonia, we should
1.
2.
3.
4.
a.
b.
c.
d.
e.
2.( A
increase the temperature.
decrease the temperature.
increase the pressure.
decrease the pressure.
1 only
2 only
1 and 3 only
2 and 3 only
1 and 4 only
) For which of the following systems at equilibrium and at constant temperature will decreasing
the volume cause the equilibrium to shift to the right?
a. N2(g) + 3H2(g)
2NH3(g)
b. 2H2O(g)
2H2(g) + O2(g)
c. 2NO2(g)
2NO(g) + O2(g)
d. NH4Cl(s)
NH3(g) + HCl(g)
e. H2(g) + Cl2(g)
2HCl(g)
3.( B
) For which of the following systems at equilibrium and at constant temperature will increasing the
volume have no effect on the equilibrium?
a. SO2Cl2(g)
SO2(g) + Cl2(g)
b. CO(g) + H2O(g)
CO2(g) + H2(g)
c. COCl2(g)
CO(g) + Cl2(g)
d. I2(g)
2I(g)
e. C(s) + CO2(g)
2CO(g)
4.( B
) In which of the following reactions does an instantaneous increase in the volume of the reaction
vessel favor formation of the products?
a. MgO(s) + CO2(g)
MgCO3(s)
b. PCl5(g)
PCl3(g) + Cl2(g)
c. H2(g) + I2(g)
2HI(g)
d. N2(g) + O2(g)
2NO(g)
e. N2(g) + 3H2(g)
2NH3(g)
5.( A
) For the following reaction system at equilibrium, which one of the changes would cause the
equilibrium to shift to the right?
Br2(g) + 2NO(g)
a.
b.
c.
d.
e.
2NOBr(g)
Decrease the volume of the reaction vessel.
Remove some NO.
Add some NOBr.
Remove some Br2.
Increase the temperature.
H° = -30 kJ
6.( E
) Consider the equilibrium
PCl3(g) + Cl2(g)
PCl5(g)
∆H = –92 kJ
The concentration of PCl3 at equilibrium will be increased by
a. increasing the pressure.
b. adding Cl2 to the system.
c. decreasing the temperature.
d. the addition of neon.
e. the addition of PCl5.
7.( E
) Solid HgO, liquid Hg, and gaseous O2 are placed in a glass bulb and are allowed to reach
equilibrium at a given temperature.
2HgO(s) + heat
2Hg(l) + O2(g)
The amount of Hg(l) in the bulb could be increased by
1.
2.
3.
a.
b.
c.
d.
e.
8.(
removing some HgO.
removing some O2.
increasing the temperature.
1 only
2 only
3 only
1 and 2 only
2 and 3 only
E ) Dinitrogen tetroxide readily undergoes decomposition to form red-brown NO2(g), as represented
by the equation
N2O4(g)
2NO2(g)
At 25°C, 0.11 mol N2O4 reacts to form 0.10 mol N2O4 and 0.02 mol NO2. At 90°C, 0.11 mol N2O4
forms 0.050 mol N2O4 and 0.12 mol NO2. From these data, we can conclude that
1.
2.
3.
a.
b.
c.
d.
e.
9.( E
N2O4 molecules react by a first-order rate law.
the reaction is endothermic.
the equilibrium constant for the reaction increases with an increase in temperature.
1 only
2 only
3 only
1 and 2 only
2 and 3 only
) If the system NH4Cl(s)
NH3(g) + HCl(g) is at equilibrium at constant temperature and the
volume of the vessel is doubled, when the system comes to equilibrium,
1.
2.
3.
the amount of NH3 and HCl is doubled.
the partial pressure of NH3 and HCl in the vessel remains unchanged.
the number of moles of NH4Cl decreases.
a. 1 only
b. 2 only
c. 3 only
d. 1 and 3 only
e. 1, 2, and 3
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