The temperature dependence of the rate of a chemical equation can be accurately explained by Arrhenius equation. With the help of Arrhenius equation, calculate the rate constant for the first order reaction: `C_2H_5I(g)rarr C_2H_4(g) + HI(g)` at 700 K. Energy of activation `(E_a)` for the reaction is 209 kJ `mol^-1` and rate constant at 600 K is `1.60xx 10^-5 s^-1`. Universal gas constant, R = 8.314 `JK^-1 mol^-1`).