part a. Given the following reaction:
N2(g) + 3 H2(g) ⇌ 2 NH3(g).
When initial amounts of N2, H2, and
NH3 are mixed, the concentration of NH3 then
increases to reach equilibrium. Which statement below is
true?
Kc = Q
Kc < Q
Kc > Q
More information is needed to make a statement about Kc.
part b. Write the equilibrium expression (K) for
the forward reaction:
8 CH4 (g) + 12 O2 (g) ⇌ 8 CO (g) + 16 H2O (g)
part c. The equilibrium constant, Kp, equals 3.40 for the
reaction at 298 K. Which direction will the system shift to reach
equilibrium if a flask initially contains 1.00 atm of each
gas?
It will shift left.
The system is already at equilibrium.
It will shift right.
The system is not at equilibrium and will remain in an
unequilibrated state.
Part D Which statement is true for a reaction
with Kc equal to 8.90 × 10 -12?
The reaction is very product-favored.
The reaction is very reactant favored.
The reaction is neither product-favored nor reactant-favored
Increasing the temperature will not change the value
of Kc.
Part E Given the following reaction:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
At 250° 0.125 M PCl5 is added to the flask.
If Kc = 1.80, what are the equilibrium
concentrations of each gas?
[PCl5] = 0.0625 M, [PCl3] = 0.335 M, and [Cl2] = 0.335 M
[PCl5] = 0.00765 M, [PCl3] = 0.117 M, and [Cl2] = 0.117 M
[PCl5] = 3.96 M, [PCl3] = 3.83 M, and [Cl2] = 3.83 M
[PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M