COMEDK · Chemistry · 19. Chemical Kinetics
The hydrogenation of Ethyne is carried out at 600 K . The same reaction when carried out in presence of a catalyst maintaining the same rate constant, the temperature required is only 400 K . If the catalyst lowers the Activation energy of the reaction by \(20 \mathrm{~kJ} / \mathrm{mol}\), what is the value of \(\mathrm{E}_{\mathrm{a}}\) ?
- A \(50 \mathrm{~kJ} / \mathrm{mol}\)
- B \(80 \mathrm{~kJ} / \mathrm{mol}\)
- C \(60 \mathrm{~kJ} / \mathrm{mol}\)
- D \(100 \mathrm{~kJ} / \mathrm{mol}\)
Answer & Solution
Correct Answer
(C) \(60 \mathrm{~kJ} / \mathrm{mol}\)
Step-by-step Solution
Detailed explanation
The Arrhenius equation is given by \(k = A e^{-E_a / RT}\). For the reaction without a catalyst at \(T_1 = 600 \text{ K}\) with activation energy \(E_{a1} = E_a\), the rate constant is \(k_1 = A e^{-E_a / (R \times 600)}\). For the reaction with a catalyst at…
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