The rate constant of a first$-$order reaction is $3\mathrm{.}46{\mathrm{.}10}^{-2}{s}^{-1}$ at $298K.$ What is the rate constant at $350K$ if the activation energy for the reaction is $50\mathrm{.}2k\frac{J}{m}ol?(R=8\mathrm{.}314\frac{J}{K}.$mol $)$

$ln\frac{k_1}{k_2}=\frac{E_a}{R}(\frac{T_1-T_2}{T_1{T}_2})$

a$)1\mathrm{.}404$

b$)2\mathrm{.}602$

c$)0\mathrm{.}702$

d$)1\mathrm{.}805$

e$)0\mathrm{.}350$