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Question

For following reactions, find the activation energy for catalyzed reaction

A700KProduct

A catalyzed500KProduct

It was found that the Ea is decreased by 30KJ/mol in the presence of catalyst. If the rate remains unchanged, the activation energy for catalyzed reaction is (Assume pre exponential factor is same).


A

75kJ/mol

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B

135kJ/mol

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C

105kJ/mol

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D

198kJ/mol

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Solution

The correct option is A

75kJ/mol


The above question can be solved as:

Step 1:

T1=700K ,T2=500K

Step 2: From the formulae

K1=AeEa/RT1K1=AeEa/R700

K1=AeEa/R700K2=AeEa-30/R500

Step 3:

The rate of the reaction is same, thus K1=K2

eEa/R700=eEa-30/R500

Ea/700R=Ea-30/500R

5Ea=7Ea-210

210=2Ea

Ea=105kJ/mol

Step 3:

The activation energy of catalyzed reaction Ea-30=105-30kJ/molEa=75kJ/mol

Therefore, the activation energy of catalyzed reaction is 75kJ/mol.


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