Determine the Rate and Rate Constant CK). Equation 1: 2I'cae) + Sa Og* Cag) Iaca@)+aS0Caq) Equation 2: Rate= Egoaion 3: Rate = K[I]" [Sa0^ : ACS20,]. [7 4Cr.] [Bo7] 2At ACI] Bo] %3D 24t Fouation 4: I2 (a2) *2 SəOz*iaq)→cag) + SyO Cag) A[S.0,7 1[3305 Jorig AtSaO,-K [I[B_O/" Equaition 5: Rates - Equation6: Rate:- (rate law) Rate of lass Of reactant SaO"=Alsa05 5.00:10-M These are all of the equations given . II 1. -in order to e ion with perox- y carefully measured va,S,O, solution should be .ette. The KCl and (NH),SO, solu- -crs. Table 3: Initial Rates erefore: **Rate Constant, k **Rate Ra * [S,0,²1mt linit * [Fait init Rate Rxn # can be solved foI 0.0400M 0.0800M data from Rx 0.0400M erature, k sho trations. O.0400M O.0200M 0.0800M 0.0100M carily stain y 0.0800M 4 0.0300M 0.0600M with wate Average value for k Rate Rate Law:

Determine the Rate and Rate Constant CK). Equation 1: 2I'cae) + Sa Og* Cag) Iaca@)+aS0Caq) Equation 2: Rate= Egoaion 3: Rate = K[I]" [Sa0^ : ACS20,]. [7 4Cr.] [Bo7] 2At ACI] Bo] %3D 24t Fouation 4: I2 (a2) 2 SəOziaq)→cag) + SyO Cag) A[S.0,7 1[3305 Jorig AtSaO,-K [I[B_O/" Equaition 5: Rates - Equation6: Rate:- (rate law) Rate of lass Of reactant SaO"=Alsa05 5.00:10-M These are all of the equations given . II 1. -in order to e ion with perox- y carefully measured va,S,O, solution should be .ette. The KCl and (NH),SO, solu- -crs. Table 3: Initial Rates erefore: Rate Constant, k Rate Ra * [S,0,²1mt linit * [Fait init Rate Rxn # can be solved foI 0.0400M 0.0800M data from Rx 0.0400M erature, k sho trations. O.0400M O.0200M 0.0800M 0.0100M carily stain y 0.0800M 4 0.0300M 0.0600M with wate Average value for k Rate Rate Law:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 36QRT

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What is the difference between average rate, initial rate, and instantaneous rate?
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
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.
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
You and a coworker have developed a molecule thathas shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law Rate=k[AV]1[V]1 You have been given the following data from your coworker: [V]0=0.20M[AV]0=1.0104M A plot of ln[AV] versus t(s) gives a straight line with a slope of 0.32 s1. What is the value of the rate constant (k) for this reaction?
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
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
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 4.00 105 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 102 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 102 M C2H5OH to decompose?
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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.