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Question

A hydrogenation reaction is carried out at 500 K. If the same reaction is carried out in the presence of a catalyst at the same rate, the temperature required is 400 K. Calculate the activation energy of the reaction at 500 K, if the catalyst lowers the activation barrier by 20 kJmol−1.

A
80 kJmol1.
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B
100 kJmol1.
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C
110 kJmol1.
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D
95 kJmol1.
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Solution

The correct option is B 100 kJmol1.
Arrhenius equation is given by , k=AeEa/RT
Therefore,k500=AeE500/RT
k400=AeE400/RT
According to the question, k500=k400E500R×500=E400R×400
E5005=E4004
E500=E4004×5 ....(1)
Given, E500=E400+20 ....(2)
Substituting equation (2) in equation (1),
we get,
E400=80kJmol1
From equation (2),E500=100kJmol1

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