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# A catalyst lowers the activation energy for a certain reaction from 75 kJ to 25 kJmol−1. The effect on the rate of reaction at 25∘C, other things being equal is :rate of reaction decreases 5.81×108 timesrate of reaction decreases 6.34×108 timesrate of reaction increases 6.34×108 timesrate of reaction increases 5.81×108 times

A
rate of reaction increases 5.81×108 times
B
rate of reaction decreases 5.81×108 times
C
rate of reaction decreases 6.34×108 times
D
rate of reaction increases 6.34×108 times
Solution
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#### The relationship between the rate of the reaction and the activation energy is logk=−Ea2.303RT+logAThis equation in presence and in absence of catalyst can be written as log(k2k1)=−12.303RT(Ea2−Ea1)Here, Ea2 and Ea1 represents the activation energies in presence and in absence of catalyst and k2 and k1 represents the rate constants in presence and in absence of catalyst.Hence, log(k2k1)=−12.303×8.314×298(25000−75000)=8.763(k2k1)=5.81×108Hence, the rate of the reaction increase 5.81×108 times.

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