Question

A mixture of reactants and products has a equilibrium constant of 4.7 and initially contains 0.035 M H2O, 0.050 M CH4, 0.15 M CO, and 0.20 M H2. In which direction will the reaction go in order to attain equilibrium?

Answer 1

Answer: Reaction will move in forward direction in order to attain an equilibrium.

Explanation:

• $K_c>Q_c$  reaction will move in forward direction.

• $Q_c>K_c$  reaction will move in backward direction.

• $Q_c=K_c$  reaction is at equilibrium.

$CH_4+H_2O\rightleftharpoons CO+3H_2$

$K_{c}=4.7$

$[H_2O]=0.035 M,[CH_4]=0.050 M,[CO]=0.15 M,[H_2]=0.20 M$

The expression for equilibrium quotient is written as :

$Q_{c}=\frac{[CO][H_2]^3}{[H_2O][CH_4]}=\frac{0.15\times (0.20)^3}{0.035\times 0.050}=0.6857$

Since, $K_c>Q_c$ reaction will move in forward direction.