(D) The relationship between standard Gibbs energy change $\Delta G^{\circ}$ and equilibrium constant $K$ is given by $\Delta G^{\circ} = -RT \ln K$.A

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Assertion is incorrect but Reason is correct.

(D) The relationship between standard Gibbs energy change $\Delta G^{\circ}$ and equilibrium constant $K$ is given by $\Delta G^{\circ} = -RT \ln K$.At equilibrium,$\Delta G = 0$,but $\Delta G^{\circ}$ is not necessarily zero unless $K = 1$.Therefore,the Assertion is incorrect.However,a chemical reaction is spontaneous in the direction of decreasing Gibbs energy $(\Delta G < 0)$ at constant temperature and pressure,which makes the Reason correct.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Standard free energy

Medium

Assertion: For every chemical reaction at equilibrium,the standard Gibbs energy change is zero.
Reason: At constant temperature and pressure,a chemical reaction is spontaneous in the direction of decreasing Gibbs energy.

A
Both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
B
Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion.
C
Assertion is correct but Reason is incorrect.
D
Assertion is incorrect but Reason is correct.

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1 Equilibrium: Chemical Equilibrium

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Standard free energy

The correct relationship between the standard Gibbs free energy change $(\Delta G^o)$ and the equilibrium constant $(K_c)$ for a reaction is .......

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Which of the following expressions is correct?

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The equilibrium constant $(K)$ of a reaction may be written as :

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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 $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

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The value of $\log _{10} K$ for a reaction $A \rightleftharpoons B$ is
(Given : $\Delta _{r} H_{298 K}^{\circ} = -54.07 \ kJ \ mol^{-1}$,$\Delta _{r} S_{298 K}^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$ and $R = 8.314 \ J \ K^{-1} \ mol^{-1}$; $2.303 \times 8.314 \times 298 = 5705$)

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Assertion: For every chemical reaction at equilibrium,the standard Gibbs energy change is zero.Reason: At constant temperature and pressure,a chemical reaction is spontaneous in the direction of decreasing Gibbs energy.

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The correct relationship between the standard Gibbs free energy change $(\Delta G^o)$ and the equilibrium constant $(K_c)$ for a reaction is .......

Which of the following expressions is correct?

The equilibrium constant $(K)$ of a reaction may be written as :

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 $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

The value of $\log _{10} K$ for a reaction $A \rightleftharpoons B$ is(Given : $\Delta _{r} H_{298 K}^{\circ} = -54.07 \ kJ \ mol^{-1}$,$\Delta _{r} S_{298 K}^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$ and $R = 8.314 \ J \ K^{-1} \ mol^{-1}$; $2.303 \times 8.314 \times 298 = 5705$)

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Assertion: For every chemical reaction at equilibrium,the standard Gibbs energy change is zero.
Reason: At constant temperature and pressure,a chemical reaction is spontaneous in the direction of decreasing Gibbs energy.

The value of $\log _{10} K$ for a reaction $A \rightleftharpoons B$ is
(Given : $\Delta _{r} H_{298 K}^{\circ} = -54.07 \ kJ \ mol^{-1}$,$\Delta _{r} S_{298 K}^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$ and $R = 8.314 \ J \ K^{-1} \ mol^{-1}$; $2.303 \times 8.314 \times 298 = 5705$)