| 1. |
For the reaction2 H2S(g)
 2 H2(g) + S2(g)
at a certain temperature Kc equals 4500. What will happen
when 0.010 mole of H2S, 1.0 mole of H2, and 1.5 mole of S2
are added to a 2.0 L container and the system is brought to the temperature at which Kc
= 4500?
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a)
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Nothing, the system is at equilibrium.
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b)
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More H2S will be formed.
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c)
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More H2 will be formed than S2.
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d)
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More S2 will be formed than H2.
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e)
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The amount of H2 formed will be half the amount of S2 formed.
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| 2. |
When phosphorus pentachloride is made by the
reaction of PCl3(g) and Cl2(g) at 240oC, the Kc
= 20.PCl3(g) + Cl2(g)
PCl5(g)
If pure PCl5 is placed in a 1.00 L container and allowed to
come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.050 M,
then the concentration of PCl3(g) is:
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a)
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0.025 M.
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b)
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0.100 M.
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c)
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0.200 M.
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d)
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0.300 M.
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e)
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0.050 M.
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| 3. |
At a given temperature, 0.150 mol NO, 0.100 mol Cl2,
and 0.250 mol ClNO were placed in a 10.0-L container. The following equilibrium is
established.2 ClNO(g) 2
NO(g) + Cl2(g)
At equilibrium, 0.350 mol ClNO are present. How many moles
of Cl2 are present at equilibrium?
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a)
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0.050
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b)
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0.100
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c)
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0.150
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d)
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0.200
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e)
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0.250
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| 4. |
CS2(g)
+ 3 Cl2(g) CCl4 + S2Cl2(g)
At a given temperature the reaction above is at equilibrium when[CS2]
= 0.050 M, [Cl2] = 0.25 M, [CCl4] = 0.15 M, and [S2Cl2]
= 0.35 M. What would be the direction of the reaction when the reactants and
products have the following concentrations: CS2 = 0.15 M, Cl2
=0.20 M, CCl4 = 0.30 M, and S2Cl2 = 0.28 M?
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a)
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to the right
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b)
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to the left
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c)
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no change
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d)
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cannot predict unless we know the temperature
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e)
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cannot predict unless we know if the reaction is endothermic or exothermic
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| 5. |
0.500 mol of NOCl is placed
in a 1.00-L reaction vessel at 700 K, and after the system comes to euilibrium, the
concentration of NOCl is 0.440 M. Calculate the equilibrium constant, Kc,
for the reaction:2 NOCl(g)
2 NO(g) + Cl2(g)
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a)
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5.6 x 10-4
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b)
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2.0 x 10-3
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c)
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4.1 x 10-3
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d)
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6.1 x 10-3
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e)
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8.2 x 10-3
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