MolSynapsequestion bank

MolSynapse / Question bank / Chemical Kinetics / Arrhenius equation and activation energy

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3ck164

A reaction obeys the Arrhenius equation with $E_{a} = 50 kJ mo l^{- 1}$ ( $R = 8.314 J mo l^{- 1} K^{- 1}$ ). Which statements are correct?

AThe ratio $k_{610} / k_{600}$ is smaller than $k_{310} / k_{300}$
B $k_{310} / k_{300}$ lies between 1.8 and 2.0
CIf $E_{a}$ is doubled, the ratio $k_{310} / k_{300}$ is also doubled
DThe ratio $k_{310} / k_{300}$ does not depend on $A$

Answer: A, B, D

k_{310} / k_{300} = exp [\frac{50000}{8.314} (\frac{1}{300} - \frac{1}{310})] = 1.91

and

k_{610} / k_{600} = 1.18

, which is smaller. Doubling

E_{a}

doubles the exponent, so the ratio is squared (

3.64

), not doubled.

A

cancels in any ratio.

Practice Chemical Kinetics More on Arrhenius equation and activation energy

Previous questionNext question

More questions on Arrhenius equation and activation energy