The reaction described by this equation

o3(g)+no(> o2(g)+no2(g)

has the following rate law at 310k.

rate of reaction=k[o3][no] k=3.0*10^6m^-1*s^-1

given that [o3]=5.0x10^-4m and no=6.0x10^-5m at t=0 calculate the rate of the reaction at t=0

what is the overall order of this reaction?

Answer :

The rate of the reaction at t=0 is,

The overall order of reaction is, second order reaction.

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The general reaction is:

The general rate law expression for the reaction is:

where,

a = order with respect to A

b = order with respect to B

R = rate  law

k = rate constant

and = concentration of A and B reactant

Now we have to determine the rate law for the given reaction.

The given balanced equations is:

In this reaction, and are the reactants.

The rate law expression for the reaction is:

   ..........(1)

Given :

Rate constant =

Concentration of =

Concentration of =

Now put all the given values in equation 1, we get:

Thus, the rate of the reaction at t=0 is,

Now we have to determine the overall order of reaction.

From the given rate law expression we conclude that,

The order of reaction with respect to is, first order reaction.

The order of reaction with respect to is, first order reaction.

Thus, overall order of reaction will be:

Overall order of reaction = 1 + 1 = 2

Thus, the overall order of reaction is second order reaction.

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)