(b)The reaction between H2O2 and lodide; H,0, + 21 + 2H*→2H,0 + 12Proceeds by two parallel mechanism and led to a rate laws,k, [H,0][I] and = k, [H,0][][#*]%3DdtdtThe change in observed rate constants with ionic strength for both themechanisms is given in the following table.k (M's)0.69k2 (M's')Sr. no.Ionic strength (1)19.00.000.02070.6615.030.05250.6712.040.09250.6811.30.690.15750.20259.70.719.2With the help of this data and corresponding plots, comment on whichmechanism between these two would follow Primary salt effect moreprominently.rhich tyne of complex mechanism T-jump

Bronsted-Bjerrum equation is given as: log k =log ko + 1.02 zAzB I1/2 k = rate constant at a an…

Answered: With the help of this data and…

With the help of this data and corresponding plots, comment on which mechanism between these two would follow Primary salt effect more prominently.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.49PAE: The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by...

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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?
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.
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 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 gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for the forward reaction at 700C of 138 L/moI s and an activation energy of 165 kJ/moI. (a) Calculate the activation energy of the reverse reaction given that H f for HI is 26.48 kJ/moI and H f for I2(g) is 62.44 kJ/mol. (b) Calculate the rate constant for the reverse reaction at 700C. (Assume A in the equation k=AeE a /RT is the same for both forward and reverse reactions.) (c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
The activation energy for the decomposition of cyclobutane (C4H8) to ethylene (C2H4) is 261 kJ/mol. If the system produces ethylene at the rate of 0.043 g/s at 500C, what is the rate if the temperature increases to 600C?
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
The reaction (CH3)3CBr + OH- -> (CH3)3COH + Br- in a certain solvent is first order with respect to (CH3)CBr and zero roder with respect to OH-. In several experiemnts, the rate constant was determined at different temepratures. A plot of ln(k) vs. 1/T was constructed resulting in a straight line with a slope of -1.10x104 K and a y-intercept of 33.5 a. determine the activation energy b. determine the frequceny factor and rate constant at 25.0C c. determine the rate constant when the temperature drops to 15.0C
The reaction of ethyl acetate with sodium hydroxide, CH3 COOC,H; (aq) + NaOH(aq) = CH3COONA(aq) + C2H; OH(aq) is first order in CH3 COOC,H; and first order in NaOH. If the concentration of CH3 COOC2H; was increased by half and the concentration of NaOH was increased by four, by what factor would the reaction rate increase? Express your answer numerically.
The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3) 8.01 9.22 12.11v/(mol dm-3 s-1) (a) 125 144 190 (b) 640 730 960
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?
ssignment/takeCovalentActivity.do?1ocator=assignment-take Erro [Review Topics]) References) Use the References to access important values if needed for this question. For the gas phase decomposition of isobutyl bromide, (CH),CHCH,Br—(CH;),С-СH, + HBr the rate constant in s' has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.54×10* K and a y-intercept of 30.1. The value of the rate constant for the gas phase decomposition of isobutyl bromide at 671 K is (Enter your answer to one significant figure.) Submit Answer Retry Entire Group 8 more group attempts remaining