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  • The activation energy of a reaction at a given temperature is found to be .The rati

The activation energy of a reaction at a given temperature is found to be \mathrm{2.303RT\, Jmol^{-1}}.The ratio of rate constant to Arrhenius factor is

Option: 1

0.1


Option: 2

0.01


Option: 3

0.001


Option: 4

0.02


Answers (1)

best_answer

Arrhenius Equation -

\mathrm{k = A e^{-E_{a}/RT}}

The activation energy of a reaction at a given temperature is found to be 2.303RT J/mol.

So, Ea = 2.303RT J/mol

Now, The ratio of rate constant to Arrhenius factor is

\mathrm{\frac{k}{A} =e^{-E_{a}/RT}}

\mathrm{\frac{k}{A} =e^{-2.303RT/RT}}

\mathrm{\frac{k}{A} =e^{-2.303}}

\mathrm{\frac{k}{A} =e^{-2.303\times log 10}}

\mathrm{\frac{k}{A} =e^{-ln 10}}

\mathrm{\frac{k}{A} =e^{ln 10^{-1}}}

\mathrm{\frac{k}{A} = 10^{-1}}

\mathrm{\frac{k}{A} = 0.1}

Option 1 is correct.

 

Posted by

Devendra Khairwa

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