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The activation energy of a reaction is 75.2 kJ mol-1 in the absence of a catalyst and it lowers to 50.14 kJmol-1 with a catalyst. How many times will the rate of reaction grow in the presence of a catalyst if the reaction proceeds at 25°C ?

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 According to Arrhenius equation,

For uncatalysed reaction

=> k2/k1 = antilog (4.39)

= 2.45 x 104 

Rate of reaction increases by  2.45 x 104 times.

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