# The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reactionNO (g) + Cl2 (g) ⇄ NOCl2 (g)NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)(2b) What is the reaction intermediate in this mechanism?

Question

The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reaction
NO (g) + Cl2 (g) ⇄ NOCl2 (g)
NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)
(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)

(2b) What is the reaction intermediate in this mechanism?

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Step 1

The rate law for the 1st reaction is:

Rate = k [NO] [Cl2]

The rate law for the 2nd reaction mechanism is:

Rate = k [NO]

Step 2

The rate for 2nd reaction mechanism only depends on the concentration of nitrosyl while for 1st reaction the rate is depending on nitrosyl and chlorine both.

Step 3

The rate of 1st reaction mechanism is 2nd order while for 2nd me...

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