1.

For a reaction taking place in three steps, the rate constants are k_(1),k_(2) and k_(3). The overall rate constant is k=(k_(1)k_(2))/(k_(3)). If the energy of activation values for the first, second and third stages are 40, 50 and 60" kJ mol"^(-1) respectively, then the overall energy of activation in kJ mol"^(-1) is

Answer»

30
150
50
60

Solution :`K=(k_1k_3)/k_3`
`AE^(-E//RT)=(Ae^(-E_(1//RT))Ae^(-E_2//RT))/(Ae^(-E_3//RT))`
or`e^(-E//RT)=e^((-E_(1)-E_(2)+E_(3))//RT)`
or`-E/(RT)=(-E_1-E_2+E_3)/(RT)`
or`E=E_1+E_2-E_2=40+50-60`
`=30" kJ mol"^-1`


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