Question

The equilibrium constant for a reaction is $1\times {10}^{20}$ at $300K$. The standard Gibbs energy change for this reaction is :

• A. -115 kJ
• B. +115 kJ
• C. +166 kJ
• D. -166 kJ

Answer 1

The correct option is A -115 kJ

As we know,
$\Delta G=-2.303RT\log K_p$
$=-2.303\times 8.314\times 300\log {10}^{20}$
$=-114.88kJ$