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]

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

The mechanism involves 3 steps:

Step 1 : Fast step

Step 2: Slow step

Step 3: Fast step

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]

the answer is   c.) 1575 j.

explanation: