Question

The initial concentrations or pressure of reactants and products are given for each of the following systems. The reaction quotient and the directions in which system will shift to reach equilibrium of the following reaction is:
$2N{H}_3\left(g\right)\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right),K=17$
$\left[N{H}_3\right]=0.20M;\left[N_2\right]=1.00M;\left[H_2\right]=1.00M$

• A. 25, shifts left
• B. 25, shifts right
• C. 35, shifts left
• D. 35, shifts right

Answer 1

Answer: (A)

25, shifts left

Th expression for the reaction quotient is, $Q=\frac{\left[N_2\right][H_2{]}^3}{[N{H}_3{]}^2}=\frac{1\times 1^3}{{0.2}^2}=25$

But $K=17$, thus the value of the reaction quotient is greater than that of equilibrium constant. In other words, the concentration of products is greater than that present at the equilibrium. Hence, the equilibrium will shift to left.