The reaction -> A(aq) + B(aq) → Products(aq) was studied, and the following data were obtained: [A]o (mol/L) 0.24 0.12 0.060 0.48 [B]o (mol/L) Initial rate (mol/Los) 0.36 2.06x10-1 0.24 6.85x10-2 0.18 2.57x10-2 0.18 2.06x10-1 The rate constant for the reaction without units is

List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.

The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?

For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.

The reaction NO(g)+O3NO2(g)+O2(g) was studied by performing two experiments. In the first experiment the rate of disappearance of NO was followed in the presence of a large excess of O3. The results were as follows ([O3] remains effectively constant at 1.0 1014 molecules/cm3): Time(ms) [NO] (molecules/cm3) 0 6.0 108 100 1 5.0 108 500 1 2.4 108 700 1 1.7 108 1000 1 9.9 107 In the second experiment [NO] was held constant at2.0 1014 molecules/cm3. The data for the disappearance of O3 are as follows: Time(ms) [O3] (molecules/cm3) 0 1.0 1010 50 1 8.4 109 100 1 7.0 109 200 1 4.9 109 300 1 3.4 109 a. What is the order with respect to each reactant? b. What is the overall rate law? c. What is the value of the rate constant from each set of experiments? Rate=k[NO]xRate=k[O3]y d. What is the value of the rate constant for the overall rate law? Rate=k[NO]x[O3]y

6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5°C. Time (s) [Phenyl acetate] (mol/L) 0 0.55 15.0 0.42 30.0 0.31 45.0 0.23 60.0 0.17 75.0 0.12 90.0 0.085 Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other? What is the rate of change of the phenyl acetate concentration during the time period 60.0 seconds to 75.0 seconds? What is the instantaneous rate at 15.0 seconds?

The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.

How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.

Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.

Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?