ChemistryJEE Main 22 Jan 2026, Shift 2·Q25·Numerical·Easy–moderate

Chemical Kinetics · Arrhenius equation activation energy

Consider

\ce{A ->[$k_1$] B}

and

\ce{C ->[$k_2$] D}

are two reactions. If the rate constant (

k_1

) of the

\ce{A -> B}

reaction can be expressed by the following equation

\log_{10} k = 14.34 - \dfrac{1.5\times10^{4}}{T/\mathrm{K}}

and activation energy of

\ce{C -> D}

reaction (Ea

_2

) is

\dfrac{1}{5}

th of the

\ce{A -> B}

reaction (Ea

_1

), then the value of (Ea

_2

) is kJ mol

^{-1}

. (Nearest Integer)

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