The first order rate constant for the decompoistion of `C_(2)H_(5)I` by the reaction.
`C_(2)H_(5)I(g)rarrC_(2)H_(4)(g)+HI(g)`
at `600 K is 1.60xx10^(-5)s^(-1)`. Its energy of activation is `209 kJ mol^(-1)`. Calculate the rate constant at `700 K`

The first order rate constant for the decomposition of ethyl iodide by the reaction. C_(2)H_(2)I (g)to C_(2)H_(4) (g)+ HI (g)at 600K is 1.60 xx10^(-5)s^(-1). It is energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

The first order rate constant for the decomposition of ethyl iodide by the reaction C_2H_5I(g) rarr C_2H_4 (g) + HI(g) at 600K is 1.60 x 10^(-5) s^(-1) . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700K.

The first order rate constant for the decomposition of ethyl iodide by the reaction C_2 H_5 I_((g)) to C_2 H_4 (g) + HI_((g)) at 600 K is 1.60 xx 10^(-5) s^(-1) . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

First order rate constant for the decomposition of ethyl iodide, C_(2)H_(5)I(g)rarrC_(2)H_(4)(g)+HI(g) at 600K is 1.60xx10^(-5)s^(-1) . Its activation energy is 209kJ."mol"^(-1) . Calculate rate constant of the reaction at 700K.