Consider the following reaction at a constant temperature for which Kp = 2.7. CO
ID: 833599 • Letter: C
Question
Consider the following reaction at a constant temperature for which Kp = 2.7.
CO(g) + H2O(g) ? CO2(g) + H2(g)
If 0.153 mole of CO, 0.546 mole of H2O, 0.262 mole of CO2 and 0.743 mole of H2 are introduced into a 2 L vessel, which of the following statements will be true?
A) The system is at equilibrium and no change will occur.
B) The system is not at equilibrium and will proceed to the right to achieve equilibrium.
C) The system is not at equilibrium and will proceed to the left to achieve equilibrium.
D) The system is not at equilibrium and it cannot achieve equilibrium.
E) The system is at equilibrium, but the addition of a catalyst will cause the reaction to proceed to the right.
Explanation / Answer
Q = [CO2] [H2] / [H2O] [CO] = 0.262 x 0.743 / (0.546 x 0.153) = 2.34
Now, Kp = 2.7
Kp = Kc (RT)delta n = Kc (RT)2-2 = Kc
So, Kc = 2.7
Now, Q < Kc. Thus, equilibrium has not reached and the system will proceed to the right to achieve equilibrium.