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The reaction CHCl3(g) + Cl2(g) CCl4(g) + HCl(g) has been proposed to occur by the following mechanism. Cl2 2Cl fast equilibrium CHCl3 + Cl HCl + CCl3 slow step CCl3 + Cl CCl4 fast What is the rate law predicted by this mechanism? a. Rate = k2[CHCl3][Cl] b. Rate = kexp[CHCl3][Cl2] c. Rate = k2(k1/k-1)1/2[CHCl3][Cl2]1/2 d. Rate = k3[CCl3][Cl] e. Rate = k1[Cl2]

Respuesta :

Answer:

a. Rate = k2[CHCl3][Cl]

Explanation:

The given reaction involves the combination of trichloromethane (CHCl3) and chlorine (Cl2) to form carbon tetrachloride (CCl4) and HCl

[tex]CHCl3(g) + Cl2(g)\rightarrow CCl4(g) + HCl(g)[/tex]

The mechanism involves 3 steps:

Step 1 : Fast step

[tex]Cl2 \rightleftharpoons 2Cl[/tex]

Step 2: Slow step

[tex]CHCl3 + Cl\rightarrow CCl3 + HCl[/tex]

Step 3: Fast step

[tex]CCl3 + Cl\rightarrow CCl4[/tex]

Since the slow step is always the rate determining step, the rate of the reaction predicted by this mechanism will be determined by Step 2

i.e. Rate = k2[CHCl3][Cl]

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