For a decomposition reaction, the values of rate constant k at two different temmperature are given below: k_(1)=2.15xx10^(-8)"L mol"^(-1)s^(-1) at 650 K k_(2)=2.39xx10^(-7)"L mol"^(-1)s^(-1) at 700 K Calculate the value ofactivation energy for this reaction. [R=8.314JK^(-1)"mol"^(-1)]

For a decomposition reaction, the values of rate constant k at two dif

1.	For a decomposition reaction, the values of rate constant k at two different temmperature are given below: k_(1)=2.15xx10^(-8)"L mol"^(-1)s^(-1) at 650 K k_(2)=2.39xx10^(-7)"L mol"^(-1)s^(-1) at 700 K Calculate the value ofactivation energy for this reaction. [R=8.314JK^(-1)"mol"^(-1)]
Answer» Solution :Substitute the values in the Arrhenius equation given below: `"log"(k_(2))/(k_(1))=(E_(a))/(2.303R)[(T_(2)-T_(1))/(T_(1)T_(2))]` `"or log"(2.39xx10^(-7))/(2.15xx10^(-8))=(E_(a))/(2.303xx8.314)[(700-650)/(650xx700)]` `"ORLOG "11.116=(E_(a))/(19.147)xx(50)/(650xx700) or 1.0461=(E_(a))/(19.147)xx(50)/(455000)` or`E_(a)=(1.0461xx19.147xx455000)/(50)=182270J or 182.27kJ`