A reactant ‘A’ decomposes to produce two different products simultaneously, but at  different rate as shown below:
  $C\underset{E_2}{\overset{k_2}{\leftarrow }}A\underset{E_1}{\overset{k_1}{\to }}B$
The order of reaction is unity for both reactions and their respective rate constants  $k_1$  and  $k_2$  are $1.2\times {10}^{-2}$  and $3\times {10}^{-2}$ per second, respectively. Calculate activation energy (in  kJ/mol) for the overall reaction if the activation energy for individual steps $E_1$ and  $E_2$ are  180 and 200 kJ/mol respectively