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The first order rate constant for the de...

The first order rate constant for the decompoistion of `C_(2)H_(5)I` by the reaction.
`C_(2)H_(5)I(g)rarrC_(2)H_(4)(g)+HI(g)`
at `600 K is 1.60xx10^(-5)s^(-1)`. Its energy of activation is `209 kJ mol^(-1)`. Calculate the rate constant at `700 K`

Text Solution

Verified by Experts

We know that
`log k_(2)-logk_(1)=(E_(a))/(2.303R)[(T_(2)-T_(1))/(T_(1)T_(2))]`
`logk_(2)= logk_(1)+(E_(a))/(2.303R)[(T_(2)-T_1)/(T_(1)T_(2))]`
`= log (1.60xx10^(-5))+(209xx10^(3)Jmol)/(2.303xx8.314mol^(-1)K^(-1))xx[(100)/(600xx700)]K`
`log k_(2)= -4.796+2.599= -2.197`
`k_(2)="Antilog"(-2.197)`
`="Antilog"(-2.197+1-1)`
`="Antilog"(bar(3).803)= 6.36xx10^(-3)s^(-1)`
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