The activation energy of a first order reaction is 30 kJ/mol at 298K. The activation energy for
the same reaction in the presence of a catalyst is 24 kJ/mol at 298K. How many times the
reaction rate has changed in the presence of a catalyst?

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Solution

K = A e^-Ea/RT
First reaction
K1 = A e^-30000/RT

Second Reaction
K2 = A e^-24000/RT

take ratio of these two equations
K1/ K2 = e^-30000/RT/ e^-24000/RT
Take Ln both side
Using R = 8.314 and T = 298K

Ln(K1/K2) = -2.42
K1/K2 = 0.09
K2 = 11.24 times faster than first reaction.

Thanks.

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The activation energy of a first order reaction is 30 kJ/mol at 298K. The activation energy forthe same reaction in the presence of a catalyst is 24 kJ/mol at 298K. How many times thereaction rate has changed in the presence of a catalyst?

K = A e-Ea/RTFirst reactionK1 = A e-30000/RT Second ReactionK2 = A e-24000/RT take ratio of these two equationsK1/ K2 = e-30000/RT / e-24000/RTTake Ln both sideUsing R = 8.314 and T = 298K Ln(K1/K2) = -2.42K1/K2 = 0.09K2 = 11.24 times faster than first reaction. Thanks.

The activation energy of a first order reaction is 30 kJ/mol at 298K. The activation energy for
the same reaction in the presence of a catalyst is 24 kJ/mol at 298K. How many times the
reaction rate has changed in the presence of a catalyst?

K = A e^-Ea/RT
First reaction
K1 = A e^-30000/RT

Second Reaction
K2 = A e^-24000/RT

take ratio of these two equations
K1/ K2 = e^-30000/RT/ e^-24000/RT
Take Ln both side
Using R = 8.314 and T = 298K

Ln(K1/K2) = -2.42
K1/K2 = 0.09
K2 = 11.24 times faster than first reaction.

Thanks.