The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every `10^(@)C` rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every `10^(@)C` change in temperature. `"Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C)` Arrhenius gave an equation which describes aret constant `k` as a function of temperature `k = Ae^(-E_(a)//RT)` where `k` is the rate constant, `A` is the frequency factor or pre-exponential factor, `E_(a)` is the activation energy, `T` is the temperature in kelvin, `R` is the universal gas constant. Equation when expressed in logarithmic form becomes `log k = log A - (E_(a))/(2.303 RT)` For which of the following reactions `k_(310)//k_(300)` would be maximum?A. `P + Q rarr R, E_(a) = 10 kJ`B. `E + F rarr D, E_(a) = 21 kJ`C. `A + B rarr C, E_(a) = 10.5 kJ`D. `L+M rarr N, E_(a) = 5 kJ`