The reaction of nitrogen monoxide with ozone at 25 oC NO + O3NO2 + O2 is first order in NO and first order in O3. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =

In an experiment to determine the rate law, the rate constant was determined to be 109 M-1s-1. Using this value for the rate constant, the rate of the reaction when [NO] = 0.186 M and [O3] = 3.14×10-2 M would be [blank] Ms-1.

Answer : The value of rate of reaction is

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 given chemical equation is:

Rate law expression for the reaction is:

As per question,

a = order with respect to NO  = 1

b = order with respect to = 1

Thus, the rate law becomes:

Now, calculating the value of rate of reaction by using the rate law expression.

Given :

k = rate constant =

[NO] = concentration of NO = 0.186 M

= concentration of =

Now put all the given values in the above expression, we get:

Hence, the value of rate of reaction is

the ozone layer acts as a filter for the shorter wavelength and highly hazardous ultraviolet radiation (uvr) from the sun, protecting life on earth from its potentially harmful effects. when the sky is clear, there is an inverse relationship between stratospheric ozone and solar uvr measured at the earth's surface.