Consider this initial rate data at a certain temperature in the table for the reactionOH-(aq)[OCI¯]o[I]o[OH¯]oInitial ratesOCI" (aq) + I-(aq)→ OI (aq) + Cl(aq)Trial(М)(М)(М)(M/s)10.001870.001870.4300.00054620.001870.003500.4300.0010230.003460.001870.5760.00075340.001870.003500.6540.000671Determine the rate law.Answer Bankrate = k[OCI"][OH¯J?[I][OH¯]Determine the value of the rate constant for this reaction and the correct units.Unitsk =

Given reaction is : Experimental data is : And

Consider this initial rate data at a certain temperature in the table for the reaction OH"(aq) [OCI"], [I*], [OH¯]o Initial rates OCI" (aq) + I¯(aq) - O1- (aq) + Cl"(aq) Trial (М) (М) (М) (M/s) 1 0.00187 0.00187 0.430 0.000546 0.00187 0.00350 0.430 0.00102 3 0.00346 0.00187 0.576 0.000753 4 0.00187 0.00350 0.654 0.000671 Determine the rate law. Answer Bank rate = k [OCI"] (OH¯ [OH¯] Determine the value of the rate constant for this reaction and the correct units. Units k =

Consider this initial rate data at a certain temperature in the table for the reaction OH"(aq) [OCI"], [I*], [OH¯]o Initial rates OCI" (aq) + I¯(aq) - O1- (aq) + Cl"(aq) Trial (М) (М) (М) (M/s) 1 0.00187 0.00187 0.430 0.000546 0.00187 0.00350 0.430 0.00102 3 0.00346 0.00187 0.576 0.000753 4 0.00187 0.00350 0.654 0.000671 Determine the rate law. Answer Bank rate = k [OCI"] (OH¯ [OH¯] Determine the value of the rate constant for this reaction and the correct units. Units k =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.42QE

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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.
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 following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
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.
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
What is the difference between the integrated and differential forms of the rate law?
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?
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
Explain how a species might be part of a rate law but not part of a balanced chemical reaction.
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.