SATHEE: Chemical and Ionic Equilibrium

Chemical and Ionic Equilibrium - Result Question 69

####13. The standard Gibbs energy change at $300 K$ for the reaction, $2 A ⇌ B + C$ is 2494 . $2 J$ . At a given time, the composition of the reaction mixture is $[A] = \frac{1}{2}, [B] = 2$ and $[C] = \frac{1}{2}$ . The reaction proceeds in the

$(R = 8.314 J K / m o l, e = 2.718)$

(2015, Main)

(a) forward direction because $Q > K_{c}$

(b) reverse direction because $Q > K_{c}$

(d) reverse direction because $Q < K_{c}$

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Solution:

Given, $Δ G^{\circ} = 2494.2 J$

$Q = \frac{[B] [C]}{[A]^{2}} = \frac{2 \times \frac{1}{2}}{{(\frac{1}{2})}^{2}} = 4$

$∴$ We know, $Δ G = Δ G^{\circ} + R T \ln Q$

$\begin{aligned} = 2494.2 + 8.314 \times 300 \ln 4 & = 28747.27 J (+ ve value) \end{aligned}$

Also, we have $Δ G = R T \ln \frac{Q}{K}$

If $Δ G$ is positive, $Q > K$

Therefore, reaction shifts in reverse direction.

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Chemical and Ionic Equilibrium - Result Question 69

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