When a reaction is carried out at standard states,then at equilibrium:

The equilibrium constant for the following reaction is $K_{p} = 3.44 \times 10^{24}$ at $25 ^{\circ}C$. Calculate the value of $\Delta_{f}G^{o}(SO_2)$. Given that the value of $\Delta_{f}G^{o}(SO_3)$ is $-88.52 \ kcal/mol$. The reaction is $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

At $298 \ K$, the equilibrium constant of the process $1.5 O_{2(g)} \rightleftharpoons O_{3(g)}$ is $3 \times 10^{-29}$. The standard free energy change (in $kJ \ mol^{-1}$) of the process is approximately ($R = 8.314 \ J \ mol^{-1} \ K^{-1}$; $\log 3 = 0.47$)

The correct relationship between the standard free energy change in a reaction and the corresponding equilibrium constant $K_c$ is:

For a reaction,$\Delta G^{\circ} = -115 \, kJ$. What is the value of $\log \, K_p$ at $298 \, K$?

Identify the relation between the standard Gibbs free energy change $\Delta G^{\circ}$ and the equilibrium constant $K_c$ for a chemical reaction.