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The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine:
Step 1: Cl2(g)⇌2Cl(g)(fast)
Step 2: Cl(g)+CHCl3(g)→HCl(g)+CCl3(g)(slow)
Step 3: Cl(g)+CCl3(g)→CCl4(fast)

Part A

What is the overall reaction?

Express your answer as a chemical equation. Identify all of the phases in your answer.

Part B

What are the intermediates in the mechanism?

Express your answers as a chemical expression. If there is more then one answer, separate them by commas. Identify all of the phases in your answer.

Part G

What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)

Use a for [Cl2], b for [Cl], c for [CHCl3], d for [HCl], e for [CCl3] and k for the rate constant.

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Answer:

Overall reaction equation is:

Cl2(g) + CHCl3(g) --> HCl(g) + CCl4(g)

The intermediates are Cl(g), CCl3(g).

Rate law= ka^1/2 c

Explanation:

This reaction is a non elementary reaction. A non elementary reaction is one that does not take place in a single reactive encounter. In other words, the reaction is comprised of many steps.

The overall reaction equation is the sum of all the reaction steps after all intermediates have been cancelled out. The rate law is obtained from the slowest step in the reaction sequence.