$STATEMENT-1$: 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.
- A$STATEMENT-1$ is True,$STATEMENT-2$ is True; $STATEMENT-2$ is correct explanation for $STATEMENT-1$
- B$STATEMENT-1$ is True,$STATEMENT-2$ is True; $STATEMENT-2$ is $NOT$ a correct explanation for $STATEMENT-1$
- C$STATEMENT-1$ is True,$STATEMENT-2$ is False
- D$STATEMENT-1$ is False,$STATEMENT-2$ is True
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Calculate $\Delta G^\circ$ for the reaction, $CH_4(g) + H_2(g) \rightarrow C_2H_6(g)$ at $298 \text{ K}$, given $K_p = 2 \times 10^{17}$ and $R = 8.314 \text{ J K}^{-1} \text{mol}^{-1}$.
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View SolutionWhich of the following statements is correct for a reversible process in a state of equilibrium?
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