A reaction has both $∆$H and $∆$S negative. The rate of reaction

$∆\mathrm{G}=∆\mathrm{H}-\mathrm{T}∆\mathrm{S}$

$∆\mathrm{H}=-\mathrm{Ve} \mathrm{and}∆\mathrm{S}=-\mathrm{Ve}$

At higher temperature magnitude of $\mathrm{T}∆\mathrm{S}>∆\mathrm{H}$ ; $∆\mathrm{G}=+\mathrm{ve}$ and reaction is non-spontaneous

At low temperature magnitude of $\mathrm{T}∆\mathrm{S}<∆\mathrm{H}$ ; $∆\mathrm{G}=-\mathrm{ve}$ and reaction is spontaneous

Rate of reaction increases always with increase in temperature