Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N20, and water. 2NO(9) + H2 (9) → N,0(g) + H2O(9) In a series of experiments, the following initial rates of disappearance of NO were obtained: Initial Concentration of NO Initial Concentration of H2 Initial Rate of Reaction of NO Exp. 1 1.3 x 10-3 M 9.5 x 10-3 M 4.6 x 10-6 Ms Exp. 2 2.6 x 10-3 M 9.5 х 10-3 м 1.8 x 10-5 Ms Exp. 3 1.3 x 10-8 M 1.9 x 10-2 M 9.2 x 10-6 Ms a Find the rate law for the reaction of NO. (Use k for the rate constant.) Rate =

Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N20, and water. 2NO(9) + H2 (9) → N,0(g) + H2O(9) In a series of experiments, the following initial rates of disappearance of NO were obtained: Initial Concentration of NO Initial Concentration of H2 Initial Rate of Reaction of NO Exp. 1 1.3 x 10-3 M 9.5 x 10-3 M 4.6 x 10-6 Ms Exp. 2 2.6 x 10-3 M 9.5 х 10-3 м 1.8 x 10-5 Ms Exp. 3 1.3 x 10-8 M 1.9 x 10-2 M 9.2 x 10-6 Ms a Find the rate law for the reaction of NO. (Use k for the rate constant.) Rate =

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 5E: A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0...

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Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
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?
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?
A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
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The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
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Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.