The decomposition of A into product has value of k as `4.5xx10^(3)s^(-1) " at" 10^(@)C` and energy of activation `60"kJ.mol"^(-1)` . At what temperature would k be `1.5xx10^(4)s^(-1)` ?

Explanation

Given, `k_(1)=4.50xx10^(3)s^(-1),k_(2)=1.5xx10^(4)s^(-1)`
`T_(1)=10+273=283K, E_(a)=60"kJ.mol"^(-1)`
Applying Arrhenius equation, `E_(a)=2.303R[(T_(1)T_(2))/(T_(2)-T_(1))]log.(k_(2))/(k_(1))`
or, `log.(1.5xx10^(4))/(4.5xx10^(3))=(60000)/(2.303xx8.314)[(T_(2)-283)/(283.T_(2))]`
or, `log3.33=3133.63[(T_(2)-283)/(283T_(2))] " or, " 0.9528T_(2)=283`
`thereforeT_(2)=297K " or, "24^(@)C`