NEET Chemistry Rate of Reaction MCQ Question
If the rate constants for a reaction at 500 K and 700 K are 0.02 s^-1 and 0.07 s^-1 respectively, what is the calculated activation energy (E_a) using the given data and equation?
35.6 kJ/mol
46.2 kJ/mol
54.8 kJ/mol
62.1 kJ/mol
Correct Answer
Detailed Explanation
Using the Arrhenius equation and the provided rate constants, the activation energy (E_a) can be calculated by rearranging the formula ln(k2/k1) = (E_a/R)(1/T1 - 1/T2), substituting in the given values, and solving for E_a.
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