In order to determine the energy of activation for the decomposition of hydrogen peroxide, a student determined that the rate constant at 22.33 °C was 0.023 1/s. At 33.96 °C the rate constant increased to 0.061 1/s. What is the activation energy? A. 63 kJ/mol B. -8.1 kJ/mol C. 740 kJ/mol D. 1.3 x 10-3 kJ/mol

In order to determine the energy of activation for the decomposition of hydrogen peroxide, a student determined that the rate constant at 22.33 °C was 0.023 1/s. At 33.96 °C the rate constant increased to 0.061 1/s. What is the activation energy? A. 63 kJ/mol B. -8.1 kJ/mol C. 740 kJ/mol D. 1.3 x 10-3 kJ/mol

Name: In order to determine the energy of activation for the decomposition
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Description: In order to determine the energy of activation for the decomposition of hydrogen peroxide, a studentdetermined that the rate constant at 22.33 °C was 0.023 1/s. At 33.96 °C the rate constant increased to0.061 1/s. What is the activation energy?A. 63

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 11.51PAE: 11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant...

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The decomposition of hydrogen iodide on finely divided gold at 150C is zero order with respect to HI. The rate defined below is constant at 1.20 104 mol/L s. 2HI(g)AuH2(g)+I2(g)Rate=[HI]t=k=1.20104mol/Ls a. If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. b. How long will it take for all of the 0.250 M HI to decompose?
Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.
Would the slope of a ln(k) versus 1/T plot (with temperature in kelvin) for a catalyzed reaction be more or less negative than the slope of the ln(k) versus 1/T plot for the uncatalyzed reaction? Explain. Assume both rate laws are first-order overall.
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
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
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
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.
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
Consider the first-order decomposition of phosgene at a certain temperature. COCl2(g)productsIt is found that the concentration of phosgene is 0.0450 M after 300 seconds and 0.0200 M after 500 seconds. Calculate the following: (a) the rate constant at the temperature of the decomposition (b) the half-life of the decomposition (c) the intial concentration of phosgene

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