The decomposition of ammonia on a tungsten surface at 1100 °C NH, 1/2 N, + 3/2 H2 is zero order in NH3. In one experiment, when the initial concentration of NH was 1.11x102 M, the concentration of NH, dropped to 2.60x103 Mafter 1.85x10 seconds had passed. Based on these data, the rate constant for the reactioni

The decomposition of ammonia on a tungsten surface at 1100 °C NH, 1/2 N, + 3/2 H2 is zero order in NH3. In one experiment, when the initial concentration of NH was 1.11x102 M, the concentration of NH, dropped to 2.60x103 Mafter 1.85x10 seconds had passed. Based on these data, the rate constant for the reactioni

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 50E: The decomposition of hydrogen iodide on finely divided gold at 150C is zero order with respect to...

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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)?
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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
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.
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For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
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The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
What is the difference between average rate, initial rate, and instantaneous rate?
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?
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