Which of the following statements is correct for a reversible process in a state of equilibrium?
- A$\Delta G^{\circ} = -2.303 \, RT \log K$
- B$\Delta G^{\circ} = 2.303 \, RT \log K$
- C$\Delta G = -2.303 \, RT \log K$
- D$\Delta G = 2.303 \, RT \log K$
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Similar Questions
Consider the following reaction at $298 \ K$.
$\frac{3}{2} O_{2(g)} \rightleftharpoons O_{3(g)} ; K_{P} = 2.47 \times 10^{-29}$.
$\Delta_{r} G^{\ominus}$ for the reaction is $ . . . . . . \ kJ$. (Given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)
$\frac{3}{2} O_{2(g)} \rightleftharpoons O_{3(g)} ; K_{P} = 2.47 \times 10^{-29}$.
$\Delta_{r} G^{\ominus}$ for the reaction is $ . . . . . . \ kJ$. (Given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)
DifficultJEE MAIN 2024
View SolutionThe equilibrium constant of a reaction is related to
At $300 \ K$,$\Delta_{r} G^{\circ}$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $-11.5 \ kJ \ mol^{-1}$. The equilibrium constant at $300 \ K$ is approximately $(R=8.314 \ J \ mol^{-1} \ K^{-1})$.
The $\Delta G^o$ for the reaction $X + Y \rightleftharpoons Z$ is $-4.606 \ kcal$. The value of the equilibrium constant of the reaction at $227 \ ^oC$ is $(R = 2.0 \ cal \ mol^{-1} K^{-1})$.
Medium
View SolutionWhich condition among the following holds true at the state of half-completion for the reaction $A \rightleftharpoons B$?
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