For a decomposition, the values of rate constants at two different temperature are given below:
`k_(1) = 2.15 xx 10^(-8)L mol^(-1)s^(-1)` at 650 K
`k_(2) = 2.39 xx 10^(-7) L mol^(-1)s^(-1)` at 700 K
Calculate the value of activation energy for the reaction (R=`8.314 JK^(-1) mol^(-1))`

For a decomposition reaction, the values of rate constant k at two different temperatures are given below: K_1 = 2.15 xx 10 ^(-8) L mol^(-1) s^(-1) at 650 K K_2 = 2.39 xx 10^(-7) L mol s^(-1) at 700 K Calculate the value of activation energy for this reaction. (R = 8.314 JK ^(-1) mol^(-1) )

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

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

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

For a decomposition reaction, the values of rate constants at two different temperatures are given below: K_1 = 2.15xx10^-8 Lmol^-1s^-1 at 650k K_2 = 2.39xx10^-7 Lmol^-1s^-1 at 700k Calculate the value of activation energy for the reaction (R = 8.314 JK^-1 mol^-1 )