Problem: The reaction described by this equationO3(g) + NO(g) → O2(g) + NO2(g)has the following rate law at 310 K.rate of reaction = (3.0 x 106 M-1•s^-1)[O3][NO]Given that [O3] = 7.0 x 10-4 M and [NO] = 4.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0.What is the overall order of this reaction?

FREE Expert Solution

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

rate law=kAxBy

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


Reaction:     O3(g) + NO(g) → O2(g) + NO2(g)

Given:            [O3] = 7.0 x 10-4 M

                       [NO] = 4.0 x 10-5 M

                        k = 3.0 x 106 M-1•s-1

                       

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Problem Details

The reaction described by this equation

O3(g) + NO(g) → O2(g) + NO2(g)

has the following rate law at 310 K.

rate of reaction = (3.0 x 106 M-1•s^-1)[O3][NO]

Given that [O3] = 7.0 x 10-4 M and [NO] = 4.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0.

What is the overall order of this reaction?

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