Question

The standard Gibbs energy change at 300 $K$ for the reaction $2A\rightleftharpoons B+C$ is 2494.2 $J$. At a given time, the composition of the reaction mixture is [A] = $\frac{1}{2}$, [B] = 2 and [C] =$\frac{1}{2}$ . The reaction proceeds in the: ($R$=8.314 $J{K}^{-1}mo{l}^{-1},e=2.718$)

• A. forward direction because $Q>K_c$
• B. reverse direction because $Q>K_c$
• C. forward direction because $Q<K_c$
• D. reverse direction because $Q<K_c$

Answer 1

The correct option is B reverse direction because $Q>K_c$

We know that,

$\Delta G=\Delta G^o+RTlnQ$
=2494.2 + 8.314 $\times$300ln 4
>0 (positive)

Since $\Delta G>0$, $Q>K$, so the reaction shifts in the reverse direction