20. Use the following data to determine the reaction rate law for the reaction: 2C10220H → ClO3 + ClO2 + H2O Experiment [ClO2]0, mol/L [OH]o, mol/L Initial Rate, mol/(L´s) 1 0.050 0.100 5.75 x 102 2 0.100 0.100 2.30 x 10¹ Solve for the rate law constant, as well as the units for full marks. 3 0.100 0.050 1.15 x 10"¹

Explain how a species might be part of a rate law but not part of a balanced chemical reaction.

One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?

One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.