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The standard Gibbs energy change at 300 K for the reaction  2 A \rightleftharpoons B+C is 2494.2 J. At a given time, the composition of the reaction mixture is [A] = 1\2, [B] = 2 and [C] = 1\2. The reaction proceeds in the:

Option: 1

\text { forward direction because } Q>K_{C}


Option: 2

\text { reverse direction because } Q>K_{C}


Option: 3

\text { forward direction because } Q<K_{C}


Option: 4

\text { reverse direction because } Q<K_{C}


Answers (1)

best_answer

The standard Gibbs energy change at 300 K for the reaction  2 A \rightleftharpoons B+C 

So,

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


\\ \Delta G^{\circ} = -2.303 R T \log K_{C} \\\\ 2494.2 =-2.303 \times 8.314 \times 300 \log K_{C} \\\\ \therefore K_{C}=0.36 \\\\ \because Q>K_{C} \text { thus reaction moves in backward direction. }


Therefore,option(2) is correct

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manish painkra

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