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
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
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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