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The first order rate constant for the de...

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

Text Solution

Verified by Experts

We know that
`log k_(2)- logk_(1)=(E_(a))/(2.303R)[(1)/(T_(1))-(1)/(T_(2))]`
`log k_(2)=log k_(2) +(E_(a))/(2.303R)[(1)/(T_(1))-(1)/(T_(2))]`
`=log (1.60xx10^(-5))+(209000J mol L ^(-1))/(2.303 xx8.314 J mol L ^(-1)K^(-1))[(1)/(600K)-(1)/(700K)]`
`log k_(2)=-4.796+2.599`
`=-2.197`
`k_(2) =6.36 xx10^(-3)s^(-1)`
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