(c) At low temperatures, reaction (3) is replaced by the following reaction forming a stable dimer of CIO, which itself is rapidly photolysed to form Cl atoms: CIO + CIO Cl₂O2 2C1 + O2 Describe briefly, in qualitative terms, the effect that this reaction will have on the observed rate of ozone destruction. Note that Ka[Cl2] is the rate at which photons are absorbed by Cl2, and is often referred to as la.

The rate of a certain reaction is given by the following rate law: rate=kNO2O2 Use this information to answer the questions below. What is the reaction order in NO?   What is the reaction order in O2?   What is overall reaction order?   At a certain concentration of NO and O2, the initial rate of reaction is 8.0 x 104 M / s. What would the initial rate of the reaction be if the concentration of NO were halved? Round your answer to  2  significant digits. Ms The rate of the reaction is measured to be 0.140 M / s when [NO] = 0.65 M and [O2] = 1.7 M. Calculate the value of the rate constant. Round your answer to  2  significant digits. =k⋅M−2s−1

1. Given the following mechanism for the catalytic destruction of ozone: O3 Оз 02 + 0 O3 + 0 202 (a) Write the overall reaction. (b) What is the intermediate? Explain why. (c) Write all the rate laws for each step (in terms of [O3]). (d) The rate determining step is given as the step 2. Use the steady state approximation to derive the rate law.

The rate of a certain reaction is given by the following rate law: rate=k[H,][NH,] rate = Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in NH3? What is overall reaction order? At a certain concentration of H2 and NH3, the initial rate of M reaction is 4.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of H2 were doubled? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 50.0 M / s when [H2] = 1.7 M and [NH3] = 0.15 M. Calculate the value of the k = 0M -2 -1 •S rate constant. Round your answer to 2 significant digits.