The activation energy of a reaction at a given temperature is found to be $2.303\;R{\rm{T}}\;{\rm{ J}}\;{\rm{ mo}}{{\rm{l}}^{ - 1}}$. The ratio of rate constant to the Arrhenius factor is

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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Application +4 | -1

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

2.303\;R\mathrm{T}\;\mathrm{ J}\;\mathrm{ mo}{\mathrm{l}^{ - 1}}

. The ratio of rate constant to the Arrhenius factor is

View answer and explanation

Correct option: B

0.1

Option B (0.1) is correct because the ratio of the rate constant to the Arrhenius factor is equal to

e^{-\frac{E_a}{RT}}

, and with the given activation energy, this simplifies to

e^{-2.303} = 0.1

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\frac{1}{{{{\left[ A \right]}^2}}}

\left( {k'} \right)

\left( {k''} \right)

\left( {{{E'}_a}\;\mathrm{and}\;{{E''}_a}} \right)

30^\circ C\;to\;100^\circ C