MHT-CET

6-1.Equilibrium (Chemical Equilibrium) question bank (Chemistry)

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Q1.

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 $R = 8.314 \text{ J K}^{-1} \text{mol}^{-1}$.

(A)

$-64.695 \text{ kJ mol}^{-1}$

(B)

$-98.716 \text{ kJ mol}^{-1}$

(C)

$-44.08 \text{ kJ mol}^{-1}$

(D)

$-58.78 \text{ kJ mol}^{-1}$

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Q2.

The equilibrium constant for a reaction is $100$. What will be the value of standard Gibbs energy change at $298 \text{ K}$? $(R = 8.314 \text{ J K}^{-1} \text{mol}^{-1})$

(A)

$11.411$ \text{ kJ/mol}

(B)

$5.744$ \text{ kJ/mol}

(C)

$570.584$ \text{ kJ/mol}

(D)

$57.058$ \text{ kJ/mol}

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