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Effect of Catalyst

The rate cons...

Question

The rate constant $K_{1}$ of a reaction is found to be double that of a rate constant $K_{2}$ of another reaction. The relationship between corresponding activation energies of the two reactions at same temperature $(E_{1}$ and $E_{2})$ can be represented as:

A

E_{1} > E_{2}

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B

E_{1} < E_{2}

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C

E_{1} = E_{2}

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D

none of these

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Solution

The correct option is C $E_{1} < E_{2}$
Arrhenius equation,
$K = A e^{- E_{a} / R T}$
Larger is rate constant, lesser is energy of activation so $E_{1} < E_{2}$

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