The rate of a reaction quadruples when temperature changes from $$27^{\circ} \mathrm{C}$$ to $$57^{\circ} \mathrm{C}$$. Calculate the energy of activation.

Given $$\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6021$$

For a reaction $$3 \mathrm{~A} \rightarrow 2 \mathrm{~B}$$

The average rate of appearance of $$\mathrm{B}$$ is given by $$\frac{\Delta[B]}{\Delta t}$$. The correct relation between the average rate of appearance of $$\mathrm{B}$$ with the average rate of disappearance of A is given in option :

The correct options for the rate law that corresponds to overall first order reaction is

For a certain reaction, the rate $$=\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}]$$, when the initial concentration of A is tripled keeping concentration of $$\mathrm{B}$$ constant, the initial rate would