Problem: Consider the following mechanism for the overall reaction 2NO2Cl(g) → 2NO2(g) + Cl2(g).Step1      NO2Cl  NO2 + Cl              fastStep2     NO2Cl + Cl  NO2 + Cl2     slowIf this mechanism were correct, what would be the overall rate-law expression?A. Kc[NO2Cl]B. k2[NO2Cl]2C. k2[NO2Cl]2[Cl]D. k2KC[NO2Cl]2[Cl2]E.

FREE Expert Solution

We’re being asked to determine the overall rate-law expression for the reaction below:

2 NO2Cl(g) → 2 NO2(g) + Cl2(g)

Recall that the rate law only focuses on the reactant concentrations and has a general form of:

k = rate constant
A & B = reactants
x & y = reactant orders

When a reaction mechanism is given, the rate law can be determined using the slow step in the reaction mechanism.

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Problem Details

Consider the following mechanism for the overall reaction 2NO2Cl(g) → 2NO2(g) + Cl2(g).

Step1      NO2Cl  NO2 + Cl              fast

Step2     NO2Cl + Cl  NO2 + Cl2     slow

If this mechanism were correct, what would be the overall rate-law expression?

A. Kc[NO2Cl]

B. k2[NO2Cl]2

C. k2[NO2Cl]2[Cl]

D. k2KC[NO2Cl]2[Cl2]

E.