The rate constant of a chemical reaction at 600K is `1.6xx10^(-5)s^(-1)` . The activation energy of the reaction is `209"kJ.mol"^(-1)` . Calculate its rate constant at 700K.

Explanation

We know , `log.(k_(2))/(k_(1))=(E_(a))/(2.303R)((T_(2)-T_(1))/(T_(1)-T_(2)))(T_(2)gtT_(1))`
Given, `T_(1)=600K,k_(1)=1.6xx10^(-5)s^(-1),T_(2)=700K,k_(2)=?`
`thereforelog.(k_(2))/(1.6xx10^(-5))=(209xx10^(3))/(2.303xx8.314)((700-600)/(600xx700))`
or, `log.(k_(2))/(1.6xx10^(-5))=2.598 " or, "k_(2)=6.35xx10^(-3)s^(-1)`
`therefore ` The rate constant at `700K=6.35xx10^(-3)s^(-1)`