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When the temperature of a reaction \( A + B \rightarrow C \) is increased from \( 300\,K \) to \( 310\,K \) the rate constant increases by \( 12\% \). What is the Activation energy of the reaction?
When the temperature of a reaction \( A + B \rightarrow C \) is increased from \( 300\,K \) to \( 310\,K \) the rate constant increases by \( 12\% \). What is the Activation energy of the reaction?
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For small temperature changes, directly use Arrhenius form \( \ln(k_2/k_1) \) instead of approximationAlways convert energy to kJ/mol at the end.
Updated On: May 6, 2026
- \( 163.9 \, \text{kJ/mol} \)
- \( 85.69 \, \text{kJ/mol} \)
- \( 192.17 \, \text{kJ/mol} \)
- \( 8.76 \, \text{kJ/mol} \)
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The Correct Option is D
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