For the reaction A ⇌ B + C at equilibrium, the concentration of A is 1 × 1 0 - 3 M B is 0.15 M and C is 0.05 M. The Δ G ° for the hydrolysis of A at 300 K is - X kJ/mole. The value of X is? Report your answer by rounding it upto nearest int

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For the reaction A ⇌ B + C at equilibrium, the concentration of A is 1 × 1 0 - 3 M B is 0.15 M and C is 0.05 M. The Δ G ° for the hydrolysis of A at 300 K is - X kJ/mole. The value of X is? Report your answer by rounding it upto nearest integer.

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Correct answer: 5

As A ⇌ B + C K = B C A = 0.15 × 0.05 1 × 1 0 - 3 = 7 . 5 Δ G ° = - 2.303 R T log 10 ⁡ K e q = - 2.303 × 8.314 × 1 0 - 3 × 300 log ⁡ 7 . 5 On solving Δ G ° = - 4.99 kJ/M ≃ - 5 kJ/M So x = 5

For the reaction A ⇌ B + C at equilibrium, the concentration of A is 1 × 1 0 - 3 M B is 0.15 M and C is 0.05 M. The Δ G ° for the hydrolysis of A at 300 K is - X kJ/mole. The value of X is? Report your answer by rounding it upto nearest integer.

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