For the reaction A(g) leftharpoons 2B(g) , the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500 , - Chemistry MCQ Chemistry | ExamTest.live

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For the reaction A (g) ⇌ 2 B (g), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K .[Given : R = 0.0831 L atm mol^{- 1} K^{- 1}] K_{p} for the reaction at 1000 K is:

Solution & Step-by-step Explanation

1. Equilibrium constant K_{c} is the ratio of the forward rate constant (k_{f}) to the backward rate constant (k_{b}): K_{c} = \frac{k _{f}}{k _{b}} Given k_{b} = 2500 \times k_{f}, we have: K_{c} = \frac{k _{f}}{2500 \cdot k _{f}} = \frac{1}{2500} = 0.0004 2. The relation between K_{p} and K_{c} is: K_{p} = K_{c} (RT)^{Δ n} For the reaction A (g) ⇌ 2 B (g), Δ n = 2 - 1 = 1 .3. Substituting the values: K_{p} = 0.0004 \times (0.0831 \times 1000)^{1} = 0.0004 \times 83.1 = 0.03324 The closest value is 0.033 .

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For the reaction A (g) ⇌ 2 B (g), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K .[Given : R = 0.0831 L atm mol^{- 1} K^{- 1}] K_{p} for the reaction at 1000 K is:

83.1

2.077 \times 1 0^{5}

0.033

0.021

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