Question

Please answer #5 and #6

Ozone Decomposition: Ozone formation is faster during the day due to the action of sunlight on NO2 molecules. Thus, O.(g) accumulates in the troposphere and its concentration peaks sometime in the afternoon. During the night, ozone reacts with NO(g) according to the following reaction: NO(g) + Ox(g) = NO:(g) + Ox(). This is a single-step process with an activation energy E. = 12.5kl/mol and a AH.n=-199.5 kJ/mol. 5. Build potential energy diagram that represents the transformation of reactants to products. Indicate on the diagram the activation energy and the heat of the reaction for this process. Hour 6. Derive the rate law for this process and predict the effect on the rate of reaction of doubling og concentrations.

Answer 1

5)

The potential energy diagram for the above reaction is given below:

M Ea 12.5 xIlona K PE React arts AH = - - 199.5 kJ/onal Products Progress of Reaction

6) since it is given that the reaction is a single step process, the rate depends on both the concentraion of NO and O3.

Thus the rate law is given by [rate] = k [NO] [O3]

By doubling the concentration of [O3] the reaction rate also doubles.

----------------------------------