Assuming that energy of activation for most of the reactions is 52 (kJ), what conclusion you draw-about the effect of temperature on the rate of a reaction [Based on Arrhenius equation]

Explanation

Putting `(T)_(1)=300 (K), (T)_(2)=310 (K)`
`Ea=52,000 (Jmol)^(-1)` in the Arrhenius equation.
`log (k_(2)(k)_(1))=(Ea)(2.303R) (T_(2)-T_(1)/T _(1) T_(2)`
We get `k_(2)=k_(1)`. This shows that for `10^(circ)` rise of temperature the rate of the reaction is doubled.