NEET Chemistry Rate of Reaction MCQ Question
Given a reaction with rate constants k1 = 0.02 s^-1 at 500 K and k2 = 0.07 s^-1 at 700 K, what is the activation energy (Ea) in J/mol? Use R = 8.314 J/mol·K.
32,050 J/mol
45,750 J/mol
54,620 J/mol
62,890 J/mol
Correct Answer
Detailed Explanation
Using the Arrhenius equation in the given context, we calculate Ea using the formula: log(k2/k1) = Ea/2.303R(1/T1 - 1/T2). Substituting the values gives Ea = 32,050 J/mol.
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