NEET Chemistry Rate of Reaction MCQ Question
Given that the rate constants of a reaction are 0.02 s⁻¹ at 500 K and 0.07 s⁻¹ at 700 K, what is the activation energy (Eₐ) for this reaction in kJ/mol? (Use R = 8.314 J/mol·K)
52.5
42.0
35.5
25.7
Correct Answer
Detailed Explanation
Using the Arrhenius equation: log(k2/k1) = (Eₐ/2.303R)(1/T1 - 1/T2), solving gives Eₐ = 52.5 kJ/mol.
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