Please help + Activation Energy from Experimental DataThe iodination of acetone, CH3COCH,, in aqueous solutionis catalyzed by the hydrogen ion H+In the general rate lawrate = klg]*[H*]*[CH;COCH37what are the values of X, Y, and Z?H+I2 + CH3COCH,HI + CH;COCH,IDrag each item to the appropriate bin.> View Available Hint(s)The reaction can be followed visually by adding starch. Thepurple starch-iodine complex forms immediately, thendisappears when the iodine has been consumed. The kineticsof the reaction may be determined by recording the timerequired for the color to disappear, which is the time requiredfor the iodine, I2, to be consumed.Reset Help + Activation Energy from Experimental DataThe iodination of acetone, CH3COCH,, in aqueous solutionis catalyzed by the hydrogen ion H+In the general rate lawrate = klg]*[H*]*[CH;COCH37what are the values of X, Y, and Z?H+I2 + CH3COCH,HI + CH;COCH,IDrag each item to the appropriate bin.> View Available Hint(s)The reaction can be followed visually by adding starch. Thepurple starch-iodine complex forms immediately, thendisappears when the iodine has been consumed. The kineticsof the reaction may be determined by recording the timerequired for the color to disappear, which is the time requiredfor the iodine, I2, to be consumed.Reset Help

Introduction: We have to calculate the value of x,y,z.

he iodination of acetone, CH,COCH, in aqueous solution catalyzed by the hydrogen ion H* In the general rate law rate = KIa]*[H*]*[CH;COCH3 what are the values of X, Y, and Z? I+ CH,COCH, HI+CH,COCH,I Drag each item to the appropriate bin. > View Available Hint(s) he reaction can be followed visually by adding starch. The urple starch-iodine complex forms immediately, then lisappears when the iodine has been consumed. The kinetics of the reaction may be determined by recording the time equired for the color to disappear, which is the time required or the iodine, I, to be consumed. Reset Help

he iodination of acetone, CH,COCH, in aqueous solution catalyzed by the hydrogen ion H* In the general rate law rate = KIa][H]*[CH;COCH3 what are the values of X, Y, and Z? I+ CH,COCH, HI+CH,COCH,I Drag each item to the appropriate bin. > View Available Hint(s) he reaction can be followed visually by adding starch. The urple starch-iodine complex forms immediately, then lisappears when the iodine has been consumed. The kinetics of the reaction may be determined by recording the time equired for the color to disappear, which is the time required or the iodine, I, to be consumed. Reset Help

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 71QAP: For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation...

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For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
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
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?
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
The uncoiling of deoxyribonucleic acid (DNA) is a first-order reaction. Its activation energy is 420 kJ. At 37C, the rate constant is 4.90104min1 (a) What is the half-life of the uncoiling at 37C (normal body temperature)? (b) What is the half-life of the uncoiling if the organism has a temperature of 40C(104F)? (c) By what factor does the rate of uncoiling increase (per C) over this temperature interval?
What is the difference between average rate, initial rate, and instantaneous rate?
The first-order rate constant for the decomposition of a certain hormone in water at 25C is 3.42104day1. (a) If a 0.0200 M solution of the hormone is stored at 25C for two months, what will its concentration be at the end of that period? (b) How long will it take for the concentration of the solution to drop from 0.0200 M to 0.00350 M? (c) What is the half-life of the hormone?
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?
The following data were obtained for the gas-phase decomposition of dinitrogen pentoxide, 2N2O5(g)4NO2(g)+O2(g) [N2O5]0(mol/L) Initial Rate (mol/L s) 0.0750 8.90 104 0.190 2.26 103 0.275 3.26 103 0.410 4.85 103 Defining the rate as [N2O5]/ t write the rate law and calculate the value of the rate constant
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)?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?