The suggested mechanism for the reaction: (g) + (g) - (g) + (g), is: Step I: 2Cl (fast); Step II: + Cl -(K3)- + CCl3 (slow); Step III: CCl3 + Cl -(K4)- (fast). The experimental rate law

Question

The suggested mechanism for the reaction: $CHCl_3$(g) + $Cl_2$(g) -> $CCl_4$(g) + $HCl$(g), is: Step I: $Cl_2$ <=(K1/K2)=> 2Cl (fast); Step II: $CHCl_3$ + Cl -(K3)-> $HCl$ + CCl3 (slow); Step III: CCl3 + Cl -(K4)-> $CCl_4$ (fast). The experimental rate law consistent with the mechanism is

Prashant Kotian · Accepted Answer

Correct answer: D. The slow step is: rate = K3 [] [Cl]. From the fast equilibrium step: = [Cl]^2 / [] => [Cl] = ^(1/2) []^(1/2). Substituting [Cl] into the rate expression: rate = K3 ^(1/2) [] []^(1/2).

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