The rate of disappearance of HBr in the gas phase reaction2HBr(g) → H2(g) + Br2(g)is 0.301 M s ' at 150°C. The rate of appearance of Br2 isMs1.0.1510.09061.660.5490.602

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Answered: The rate of disappearance of HBr in the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 31QRT

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A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
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.
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
The decomposition of ozone is a second-order reaction with a rate constant of 30.6 atm1 s1 at 95 C. 2O3(g)3O2(g) If ozone is originally present at a partial pressure of 21 torr, calculate the length of time needed for the ozone pressure to decrease to 1.0 torr.
When heated, tetrafluoroethylene dimerizes to form octafluorocyclobutane. C2F4(g) C4F8(g) To determine the rate of this reaction at 488 K, the data in the table were collected. Analysis was done graphically, as shown below: (a) What is the rate law for this reaction? (b) What is the value of the rate constant? (c) What is the concentration of C2F4 after 600 s? (d) How long will it take until the reaction is 90% complete?
Nitrogen monoxide reacts with hydrogen as follows: 2NO(g)+H2(g)N2O(g)+H2O(g) The rate law is [H2]/t = k[NO]2[H2], where k is 1.10 107 L2/(mol2 s) at 826C. A vessel contains NO and H2 at 826C. The partial pressures of NO and H2 are 144 mmHg and 315 mmHg, respectively. What is the rate of decrease of partial pressure of NO? See Problem 13.151.
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 reaction has two reactants Q and P. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expressions? (a) rate=k1(b) rate=k2[ P ]2[ Q ] (c) rate=k3[ Q ]2 (d) rate=k4[ P ][ Q ]

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The rate of disappearance of HBr in the gas phase reaction 2HB1(g) → H2(g) + Br2(g) is 0.301 M s1 at 150°C. The rate of appearance of Br2 is Ms1. 0.151 0.0906 O 1.66 0.549 0.602