The temperature dependence of the rate of achemical reaction 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)toC_2H_(4(g))+HI_((G))at700K.Energy of activation (Ea)for the reaction is 209kjmol_(-1)and rate constant at 600K is 1.60xx10^(-5)s^(-1)[Universal gas constant R=8.314JK^(-1)mol^(-1)]

The temperature dependence of the rate of achemical reaction can be ac

1.	The temperature dependence of the rate of achemical reaction 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)toC_2H_(4(g))+HI_((G))at700K.Energy of activation (Ea)for the reaction is 209kjmol_(-1)and rate constant at 600K is 1.60xx10^(-5)s^(-1)[Universal gas constant R=8.314JK^(-1)mol^(-1)]
Answer» Solution :log `k_2= log(1.60xx10^(-5))+(209xx10^3Jmol^(-3)XX100)/(2.303xx8.314xx600xx700)=(0.204-5)+2.599=-2.197` `therfore k_2`=antilogo-2.197=antilogoof3.803=`6.3535xx10^(-3)s^(-1)`