Question

The equilibrium constant $K_p$ for a homogeneous gaseous reaction is ${10}^{-8}$. The standard Gibbs free energy change $\Delta G^{\ominus }$ for the reaction (using $R=2cal{K}^{-1}mo{l}^{-1})$ is:

• A. $10.98kcal$
• B. $-1.8kcal$
• C. $-4.1454kcal$
• D. $+4.1454kcal$

Answer 1

Answer: (A)

$10.98kcal$

$\Delta G^{\ominus }=-2.303RTlogK$

$=-2.303\times 2\times 298log{10}^{-8}$

$=-2.303\times 2\times 298\times -8cal$

$=10980cal=10.98kcal$