$k=Ae^{\frac{E_a}{RT}}$
where,
$k =$ rate constant of a chemical reaction
$E _{ a }=$ Activation energy.
$R =$ Universal gas constant
$A=$ Pre-exponential factor
From this, we can easily infer that the value of the equilibrium constant depends only on the temperature.
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$CH_3CH=CHCH_2CHBrCH_3$
$ \text { a } \mathrm{Cl}_2(\mathrm{~g})+\mathrm{b} \mathrm{OH}^{-}(\mathrm{aq}) \rightarrow \mathrm{c} \mathrm{ClO}^{-}(\mathrm{aq})+\mathrm{d} \mathrm{Cl}^{-}(\mathrm{aq}) +\mathrm{e} \mathrm{H}_2 \mathrm{O}(l)$
The values of $a, \ b,\ c$ and $d$ in a balanced redox reaction are respectively :