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At 27b0C in presence of a catalyst, activation energy of a reaction is lowered by 10 kJ mol^-1. The logarithm ratio of k (catalysed) / k (uncatalysed) is ........ (Consider that the frequency factor for both the reactions is same)

1. 17.41
2. 1.741
3. 3.482
4. 0.1741

Correct answer: 1.741

Solution

The logarithm ratio of the rate constants can be calculated using the Arrhenius equation, which shows that a decrease in activation energy leads to an exponential increase in the rate constant. Given the reduction of 10 kJ/mol in activation energy, the resulting ratio of the rate constants is approximately 1.741, indicating a significant increase in reaction rate due to the catalyst.

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