The following data were collected for the reaction 3 A(g) + 2 B (g) → 5 C(g). What is the rate law for the reaction? [B]o Experiment [Alo(M) (M) Rate (M/s) 1 1.40 1.72 0.5556 2 1.40 5.84 21.74 2.60 1.72 1.916 Rate=k [A]?[B]3 Rate=k [A]°[B]? Rate=k [A]°[B]5 Rate=k [A]?[B]? Rate=k [A]*[B]1 Rate=k [A][B]4

The following data were collected for the reaction 3 A(g) + 2 B (g) → 5 C(g). What is the rate law for the reaction? [B]o Experiment [Alo(M) (M) Rate (M/s) 1 1.40 1.72 0.5556 2 1.40 5.84 21.74 2.60 1.72 1.916 Rate=k [A]?[B]3 Rate=k [A]°[B]? Rate=k [A]°[B]5 Rate=k [A]?[B]? Rate=k [A]*[B]1 Rate=k [A][B]4

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 11.32PAE: 11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1)...

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In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were obtained: Initial Concentration of Azomethane Initial Rate Exp. 1 1.13 102 M 2.8 106 M/s Exp. 2 2.26 102 M 5.6 106 M/s What is the rate law? What is the value of the rate constant?
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
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The decomposition of nitrosyl chloride was studied: 2NOCl(g) 2NO(g) + Cl2(g) The following data were obtained where Rate=[NOCl]t [NOCl]0(molecules/cm3) Initial Rate (molecules/cm3 s) 3.0 1016 5.98 104 2.0 1016 2.66 104 1.0 1016 6.64 103 4.0 1016 1.06 105 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the value of the rate constant when concentrations are given in moles per liter.
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?
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature: Time(s) [H2O2](mol/L) 0 1.00 120 1 0.91 300 1 0.78 600 1 0.59 1200 1 0.37 1800 1 0.22 2400 1 0.13 3000 1 0.082 3600 1 0.050 Assuming that Rate=[H2O2]t determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [H2O2] at 4000. s after the start of the reaction.
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Given the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same? (a) Cl2+COCI2COrate=k[ CI2]3/2[CO] (b) PCI3+CI2PCI5rate=k[PCI3][CI2] (c) 2NO+H2N2+H2Orate=k[NO][H2] (d) 2NO+O22NO2rate=k[NO]2[O2] (e) NO+O3NO2+O2rate=k[NO][O3]