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InterviewSolution
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Write a stoichiometric equation for the reaction between `A_(2)` and `C` whose mechanism is given below. Determine the value of equilibrium constant for the first step. Write a rate law equation for the over all reaction in terms of its initial reactants. (`i`) `A_(2)overset(K_(1))underset(K_(2))hArr2A` `K_(1)=10^(10)s^(-1)` and `K_(2)=10^(10)M^(-1)s^(-1)` (`ii`) `A+CtoAC` `K=10^(-4)M^(-1)S^(-1)` |
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Answer» It is apparent from both the steps that step (`ii`) is slowest and thus `Rate=K[A][C]` ….(`1`) However overall rate constant `K` can be obtained in terms of `A_(2)` as follows, `eq.(`i`)+2xxeq.(`ii`)`, `A_(2)+2Cto2AC` Also for step (`i`), `K_(c)=(K_(1))/(K_(2))=([A]^(2))/([A_(2)])=(10^(10))/(10^(10))=1` or `[A_(2)]=[A]^(2)` or `[A]=[A_(2)]^(1//2)` Thus by eq. (`1`), `Rate=K[C][A_(2)]^(1//2)` `=K[C][A_(2)]^(1//2)` |
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