An important reaction in the formation of photochemical smog is the reaction between ozone and NO:

NO(g)+O3(g)--> NO2(g)+O2(g)

The reaction is first order in NO and O3. The rate constant of the reaction is 80 (1/Ms) at 25 C and 3.000 x 10^3 (1/Ms) at 75 C.

(a) If this reaction were to occur in single step, would the rate law be consistent with the observed order of the reaction for NO and O3? yes/no

(b) What is the value of the activation energy of the reaction?

(c) What is the rate of the reaction at 25 X when [NO]= 2.63 x 10^-6 M and [O3]=5.96 x 10^-9 M?

(d) Predict the values of the rate constant at the following temperatures:

10 C and 35 C

Question

An important reaction in the formation of photochemical smog is the reaction between ozone and NO:

NO(g)+O3(g)--> NO2(g)+O2(g)

The reaction is first order in NO and O3. The rate constant of the reaction is 80 (1/M*s) at 25 C and 3.000 x 10^3 (1/M*s) at 75 C.

(a) If this reaction were to occur in single step, would the rate law be consistent with the observed order of the reaction for NO and O3? yes/no

(b) What is the value of the activation energy of the reaction?

(c) What is the rate of the reaction at 25 X when [NO]= 2.63 x 10^-6 M and [O3]=5.96 x 10^-9 M?

(d) Predict the values of the rate constant at the following temperatures:

10 C and 35 C

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