The decomposition of N₂O5 can be described by the equation2N₂O,(soln)→ 4NO₂ (soln) + O₂(g)▷RVConsider the data in the table for the reaction at 45 °C in carbon tetrachloride solution.D%5TGt (s)B0205406755Given the data, calculate the average rate of reaction for each successive time interval.D0.What is the average rate of reaction for the time interval from 0 s to 205 son Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry Publisher: Univers?aG66°F6YH&7[N₂O5] (M)U2.5332.227N M1.9621.5758|K9f10OoL>112presented by Macmi+[||insertt]pauseprt scbackspa What is the average rate of reaction for the time interval from 0 s to 205 s?$average rate of reaction:R0What is the average rate of reaction for the time interval from 205 s to 406 s?average rate of reaction:de%5What is the average rate of reaction for the time interval from 406 s to 755 s?TIncorrectaverage rate of reaction:GB1.49 x10a6IncorrectHY1.32 ×10-3-323N0.0011Incorrect&UJ8M19K<9f10OLQuestion Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books66°F A())6:20 PM9/28/2022O>(124+[||insert]FeedbackM/spauseM/s1prt scbackspaceM/sdeletehenter↑

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The decomposition of N₂O5 can be described by the equation 2N₂O, (soln) -> 4 NO₂ (soln) + O₂(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. R % 48 5 T t (s) G 0 205 406 755 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time Y & 7 с [N₂O5] (M) H J 2.533 2.227 1.962 1.575 00 V B N M interval from 0 s to 205 88on Source: McQuarrie, Rock, And Gallogly 4e-General Chemistry 66°F к ho O ▶11 ▶I P presented by Macm { insert Publisher: Univer pause 9/2 prt sc backspa

The decomposition of N₂O5 can be described by the equation 2N₂O, (soln) -> 4 NO₂ (soln) + O₂(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. R % 48 5 T t (s) G 0 205 406 755 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time Y & 7 с [N₂O5] (M) H J 2.533 2.227 1.962 1.575 00 V B N M interval from 0 s to 205 88on Source: McQuarrie, Rock, And Gallogly 4e-General Chemistry 66°F к ho O ▶11 ▶I P presented by Macm { insert Publisher: Univer pause 9/2 prt sc backspa

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 37E: The decomposition of hydrogen peroxide was studied, and the following data were obtained at a...

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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
Hydrogen peroxide in aqueous solution decomposes by a first-order reaction to water and oxygen. The rate constant for this decomposition is 7.40 104/s. What quantity of heat energy is initially liberated per second from 2.00 L of solution that is 1.50 M H2O2? See Appendix C for data.
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?
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 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
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 initial rate ( [NO]/ t] of the reaction of nitrogen monoxide and oxygen NO(g) + 2O2(g) NO2(g) was measured for various initial concentrations of NO and O2 at 25 C. Determine the rate equation from these data. What is the value of the rate constant, k, and what are its units?
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.
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 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.