The chlorine-atom-catalyzed chlorination of methane is thought to proceed by a t

Question

The chlorine-atom-catalyzed chlorination of methane is thought to proceed by a two-step mechanism:

CH4(g) + Cl(g) --> CH3(g) + HCl(g) (slow)
CH3(g) + Cl2(g) --> CH3Cl(g) + Cl(g)

1) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process.

A) Rate = k [CH4] [Cl2]
B) Rate = k [CH3] [Cl2]
C) Rate = k [CH4]2
D) Rate = k [CH4]2 [Cl2]
E) Rate = k [Cl] [CH4]
F) Rate = k [Cl] [CH3]

2) Choose the correct chemical equation for the overall process.

A) CH4(g) + Cl2(g) --> CH3Cl(g) + HCl(g)
B) CH4(g) + Cl(g) --> CH3(g) + HCl(g)
C) CH3(g) + Cl2(g) --> CH3Cl(g) + Cl(g)

3) Identify an intermediate in the reaction.

A) CH4
B) CH3
C) Cl
D) CH3Cl

I think number one is B but I'm not sure.

Explanation / Answer

a)Rate = k[CH4][Cl2] b)CH4 + 2 Cl2 ---> CH3Cl + Cl + HCl

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