The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH (CH)3COН + Br Experiment [(CH3)3CB1],. M [OH], M Initial Rate, Ms1 6.64x10-3 6.64x10-3 1.33x10-2 1.33x10-2 1 0.540 0.408 0.540 0.816 1.08 0.408 1.08 0.816 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH (CH)3COН + Br Experiment [(CH3)3CB1],. M [OH], M Initial Rate, Ms1 6.64x10-3 6.64x10-3 1.33x10-2 1.33x10-2 1 0.540 0.408 0.540 0.816 1.08 0.408 1.08 0.816 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter30: Kinetic Methods Of Analysis

Section: Chapter Questions

Problem 30.6QAP

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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.
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?
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
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO2g+F2g)->NO2F(g)+F(g) k1 2 F(g)+NO2(g)->NO2F(g) k2 Suppose also k1 ≪ k2. That is, the first step is much slower than the second.
The second-order rate constant for the reaction CH3COOC2H5(aq) + OH-(aq)→ CH3CO2-(aq) + CH3CH2OH(aq) is 0.11 dm3 mol-1 s- 1. What is the concentration of ester after(a) 15 s, (b) 15 min when ethyl acetate is added to sodium hydroxide so that the in it ial concentrations are [NaOH] 0.055 mol dm-3 and [CH3COOC2H5] = 0.150 mol dm-3?
(i) In an iodine-clock involving peroxide: H2O2 (aq) +2I- (aq) + 2H+(aq) → 2H2O(l) + I2 (aq) The rate law has been determined to be: rate = k [H2O2][I-] with k= 0.658 L/Ms at 250C. If [I-] = 0.5, [H2O2]=0.25 and pH=5 what is the rate of reaction? (ii) In “peroxide clock” reaction above what is the rate of loss of I- ?
The second-order rate constant for the reaction CH3COOC2H5 (aq) + OH- (aq) →CH3CO2- (aq) + CH3CH2OH (aq) Is 0.11 dm3.mol-1.s-1. What is the concentration of ester after 10 minutes when ethyl acetate is added to sodium hydroxide so that the initial concentrations are 0.050 M and 0.100 M for sodium hydroxide and ethyl acetate, respectively?
1. The following initial rate data are for the ozonization of pentene in carbon tetrachloride solution at 25 oC:C5H10 + O3 C5H10O3 Experiment [C5H10]o, M [O3]o, M Initial Rate, Ms-1 1 6.32×10-2 1.34×10-2 76.0 2 6.32×10-2 2.68×10-2 152 3 0.126 1.34×10-2 151 4 0.126 2.68×10-2 303 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is ________ M-1s-1.
Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1. If k1 = 5.9×10-5 Lmol-1s-1 and Keq = 0.27 what is k-1 for a solution originally prepared with [A]0 = 0.123 molL-1 and [D]0 = 0?
Table 1 with temperature and rate constants Temperature (oC) Rate constants KH (min-1) 61.0 7.13*10-6 71.2 2.77*10-5 Mark and Anthony have considered the following reaction for urea NH2CONH2 in 0.1M HCl: NH2CONH2 + 2H2O --> 2NH+2 + CO2-3 and the rate constant for the reaction is k1. Stephan and Kurt have been in the laboratory and measured rate constants for the reaction at two different temperatures. The measurement results are given in Table 1. 1) You must write down expressions for the changes in time for the concentrations of the reactants and products. That is, determine d[X]/dt, where [X] is the concentration of either reactants or products and write this down using concentrations and the rate constant. 2) You must use the Arrhenius expression to determine the activation energy for the reaction. 3) You must use the Arrhenius expression to determine the pre-exponential factor in the Arrhenius expression.
Q4. Your report must include clearly labelled plots you have used to make the determination of the reaction order. Compare R2 values
For the gas phase decomposition of dimethyl ether at 500 °CCH3OCH3CH4 + H2 + COthe following data have been obtained: [CH3OCH3], M 0.123 7.49×10-2 4.56×10-2 2.78×10-2 time, min 0 20.7 41.4 62.1 The average rate of disappearance of CH3OCH3 over the time period from t = 0 min to t = 20.7 min is ___________M min-1.