6. 0.156 = k [0.000255) 2. The catalyzed decomposition of hydrogen peroxide, H₂O2(aq), is represented by the following equation. -0.05 2 H₂O2(sq) 2 H₂O(L) + O2(g) -0.06 0.11 The kinetics of the decomposition reaction were studied and the analysis of the results show that it is a first-order reaction. Some of the experimental data are shown in the table to the right. ola catalyst 0/2 (a) During the analysis of the data, the graph to the right was produced. Label the vertical axis of this graph. Dash in a second line that represents the plot of the uncatalyzed first-order decomposition of 1.00 M H₂O2(aq). 0.22 - 0.17 concentration. 6253444 mol L-1 rate = k 0.6084 [H₂O₂] (mol L ¹) 1.00 0.78 (13 0.61 0.50 time (minutes) suse your Integrated rate (b) Use the data in the table to calculate the rate constat, k, and specify the units. Be sure to show the method you used in your calculations. laws! = 1 (5) 2 rate = k [H₂0₂] ² rate = K [1.00]² nate = k 1 rate = k [1.00] 1 Time (minutes) 1 (0.78] 5.0 10.0 ? rate=1 [0.78] ² rate -1 [2084] (c) Calculate the time that is missing from the table. Be certain to show all work you used to make this calculation. 0/2 Juster 45 +5 +5 1 - 1.28705 = 1(5) -0.28 205 = k/s) 5 B 12=-0.06

The isomerization reaction CH3NCCH3CN obeys the first-order rate law rate=k[CH3NC] in the presence of an excess of argon. Measurementsat500 K reveal that in 520 s theconcentration of CH3NC decreases to 71% of its original value. Calculate the rateconstant k of the reaction at 500 K.

For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.

The gas-phase reaction of nitrogen monoxide with chlorine proceeds to form nitrosyl chloride. 2NO(g)+Cl2(g)2NOCl(g)rate=k[NO]2[Cl]2 Evaluate the following proposed mechanism to determine whether it is consistent with the experimental results, and identify intermediates, if any. 2NOk1k1N2O2Fast,reversibleN2O2(g)+Cl2(g)2NOCl(g)Slow(rate-limiting)step

What is the difference between the integrated and differential forms of the rate law?

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.

The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.

A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?

Derive an expression for the half-life of a a third order reaction;b a reaction whose order is =1; c a reaction whose order is 12. In these last two cases, examples are rare but known.

The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?