The reaction quotient, Q, is useful in determining if a chemical reaction is at equilibrium.
Concept #1: Comparing Q to K determines which direction the reaction shifts in order to reach equilibrium.
When Q = K then our chemical reaction is at equilibrium and no shifting will occur.
If Q is larger than K then the reaction will shift in the reverse direction to attain equilibrium.
If Q is smaller than K then the reaction will shift in the forward direction to attain equilibrium.
Example #1: Consider the hypothetical reaction below
3 A (g) + B (g) ↔ 2 C (g) Kc = 1.5 x 10-3
Which of the following statements is correct if the initial concentrations are [A] = 0.85 M, [B] = 0.36 M, and [C] = 0.005 M.
A. At equilibrium, the amount of C will increase.
B. At equilibrium, the amount of A will increase.
C. At equilibrium, the amount of B will increase and C will increase.
D. At equilibrium, the amount of A will increase and B will decrease.
E. The reaction is at equilibrium.
Example #2: For the reaction: 2 CO2 (g) 2 CO g) + 2 O2 (g), the equilibrium constant is 7.22 x 10-4 at 400 K, while the reaction quotient is 6.63 x 10-2. If initially we have 0.20 atm CO2, 0.30 atm CO and 0.15 atm O2, which of the following statements is not true?
a) The pressure of CO2 will be greater than 0.20 atm.
b) The pressure of CO will be less than 0.30 atm.
c) The pressure of O2 will be greater than 0.15 atm.
d) The pressure of O2 will be less than 0.15 atm.
e) The reaction will favor reactants.
Example #3: For the following reaction:
3 H2 (g) + N2 (g) 2 NH3 (g)
Keq = 25. At a particular time, the following concentrations are measured for the given compounds: [H2] = 0.005 M, [N2] = 0.170 M and [NH3] = 3.12 x 102 M. Which of the following statements is true?
a) The concentration of H2 will increase.
b) The equilibrium constant will increase.
c) The concentration of NH3 will increase.
d) The concentration of N2 will decrease.
e) No change will occur.