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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The equilibrium constant of a reaction is $0.008$ at $298 \ K$. The standard free energy change of the reaction at the same temperature is
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View SolutionDescribe the relationship between Gibbs energy change and chemical equilibrium.
Difficult
View Solution$STATEMENT-1$: For every chemical reaction at equilibrium,standard Gibbs energy of reaction is zero. $STATEMENT-2$: At constant temperature and pressure,chemical reactions are spontaneous in the direction of decreasing Gibbs energy.
Find the value of the equilibrium constant $(K)$ of a reaction at $300 \ K$, when standard Gibbs free energy change is $-25 \ kJ \ mol^{-1}$? (Consider $R = 8.33 \ J \ mol^{-1} \ K^{-1}$)
The equilibrium constant for a reaction is $20$. What is the value of $\Delta G^{\circ}$ at $300 \ K$? (Given: $R = 8 \times 10^{-3} \ kJ \ K^{-1} \ mol^{-1}$,$\ln(20) \approx 2.996$)
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