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The first order rate constant for the de...

The first order rate constant for the decomposition 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

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