The following data were obtained when the gas-phase reaction represented by the equation: 2 A + B → C + D was studied at 25 °C. Initial Rate Initial [B] Initial [A] (М) of Formation of C Trial (М) (Ms-1) I 0.25 0.75 4.3 х 104 II 0.75 0.75 1.3 x 10-3 III 1.50 1.50 5.3 х 10-3 a. Determine the order of the reaction with respect to reactants A and B. Justify your answer. b. Give the rate law for the reaction. Calculate the value of the rate constant, k, and specify the units of k.

The following data were obtained when the gas-phase reaction represented by the equation: 2 A + B → C + D was studied at 25 °C. Initial Rate Initial [B] Initial [A] (М) of Formation of C Trial (М) (Ms-1) I 0.25 0.75 4.3 х 104 II 0.75 0.75 1.3 x 10-3 III 1.50 1.50 5.3 х 10-3 a. Determine the order of the reaction with respect to reactants A and B. Justify your answer. b. Give the rate law for the reaction. Calculate the value of the rate constant, k, and specify the units of k.

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 26QAP: When nitrogen dioxide reacts with carbon monoxide, the following reaction occurs. Â...

See similar textbooks

Similar questions

The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
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.
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
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?
Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
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.
Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 102 mol sulfuryl chloride was heated to 600. K in a 5.00 101-L container. Time (hours): 0.00 1.00 2.00 4.00 8.00 16.00 PSO2Cl2(atm): 4.93 4.26 3.52 2.53 1.30 0.34 Defining the rate as [SO2Cl2]t, a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K. b. what is the half-life of the reaction? c. what fraction of the sulfuryl chloride remains after 20.0 h?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.