Consider the reaction between hydrogen (H2(g)) and iodine (I2(s)). The rate constant2.45 x 104 M-1s-1 for the reaction taking place at 302°C, and 0.950 M-1s-1 at 508°C.a) What is the order of the reaction? Justify your answer.b) Calculate the activation energy for this reaction.c) At 400°C what fraction of molecules have an energy greater than the activationenergy?

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Answered: Consider the reaction between hydrogen…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 57AP

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11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
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)?
The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and the half-life is 30.0 s. Calculate the concentration of the reactant exactly 60 s after initiation of the reaction. How long would it take for the concentration of the reactant to drop to one-eighth its initial value? How long would it take for the concentration of the reactant to drop to 0.040 mol/L?
The decomposition of sulfuryl chlorideSO2Cl2fur dioxide and chlorine gases is a first-order reaction. It is found that at a certain temperature, it takes 1.43 hours to decompose 0.0714 M to 0.0681 M. (a) What is the rate constant for the decomposition? (b) What is the rate of decompostion [ SO2Cl2 ]=0.0462M? (c) How long will it take to decompose SO2Cl2 so that 45% remains?
At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.
For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
A popular chemical demonstration is the magic genie procedure, in which hydrogen peroxide decomposes to water and oxygen gas with the aid of a catalyst. The activation energy of this (uncatalyzed) reaction is 70.0 kJ/mol. When the catalyst is added, the activation energy (at 20.C) is 42.0 kJ/mol. Theoretically, to what temperature (C) would one have to heat the hydrogen peroxide solution so that the rate of the uncatalyzed reaction is equal to the rate of the catalyzed reaction at 20.C? Assume the frequency factor A is constant, and assume the initial concentrations are the same.
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
As with any drug, aspirin (acetylsalicylic acid) must remain in the bloodstream long enough to be effective. Assume that the removal of aspirin from the bloodstream into the urine is a lirst-order reaction, with a half-life of about 3 hours. The instructions on an aspirin bottle say to take 1 or 2 tablets every 4 hours. If a person takes 2 aspirin tablets, how much aspirin remains in the bloodstream when it is time for the second dose? (A standard tablet contains 325 mg of aspirin.)
Chlorine dioxide oxidizes iodide ion in aqueous solution to iodine; chlorine dioxide is reduced to chlorite ion. 2ClO2(aq)+2I(aq)2ClO2(aq)+I2(aq) The order of the reaction with respect to ClO2 was determined by starting with a large excess of I, so that its concentration was essentially constant. Then Rate=k[ClO2]m[I]n=k[ClO2]m where k= k[I]n. Determine the order with respect to ClO2 and the rate constant k by plotting the following data assuming first- and then second-order kinetics. [Data from H. Fukutomi and G. Gordon, J. Am. Chem. Soc., 89, 1362 (1967).] Time (s) [ClO2] (mol/L) 0.00 4.77 104 1.00 4.31 104 2.00 3.91 104 3.00 3.53 104 5.00 2.89 104 10.00 1.76 104 30.00 2.4 105 50.00 3.2 106
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.

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