The standard Gibbs energy change at 300 K for the reaction $2\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$ is 2494.2 J. At a given time, the composition of the reaction mixture is $\left[\mathrm{A}\right]=\frac{1}{2},\mathrm{ }\left[\mathrm{B}\right]=2$ and $\left[\mathrm{C}\right]=\frac{1}{2}$ . The reaction proceeds in the: $[\mathrm{R}=8.314\mathrm{ }\mathrm{J}/\mathrm{K}-\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ },\mathrm{ }\mathrm{ }\mathrm{e}=2.718]$ {Given antilog (-0.44)=0.36}

• A

  Reverse direction because $\mathrm{Q}<{\mathrm{K}}_{\mathrm{C}}$
• B

  Forward direction because $\mathrm{Q}>{\mathrm{K}}_{\mathrm{C}}$
• Correct answer
  C

  Reverse direction because $\mathrm{Q}>{\mathrm{K}}_{\mathrm{C}}$
• D

  Forward direction because $\mathrm{Q}<{\mathrm{K}}_{\mathrm{C}}$

Hence, the correct answer is option: 'C'.