The saponification reaction of ethyl acetate $($B$)$ with NaOH $($A$)$ is carried out in a batch reactor

under isothermal conditions and at constant volume of $1$L$.$ Each reactant is used in equal volume

$(500$ mL$)$ and initial concentration $(0\mathrm{.}1$M$).$ The rate constants at $30\backslash$deg C $($k$1)$ and $40\backslash$deg C $($k$2)$ are

found to be $0\mathrm{.}010$ L$/$mol$.$s and $0\mathrm{.}021$ L$/$mol$.$s$,$ respectively. The ideal gas constant value is given

below. $($R$=8\mathrm{.}314$ J$/$mol$.$K$)$

According to this,

a$)$ Calculate the Activation energy of the reaction $($Ea$,$ kJ$/$mol$)$ from the two temperatures.

b$)$ Calculate the Pre$-$exponential factor of the reaction $($k$0,$ L$/$mol$.$s$).$

c$)$ What is the initial concentration $($CA$0$ or CB$0)$ of one of the reactants $($Ethyl acetate or NaOH$)$

when mixed even if it is not possible to measure?