For the gas phase decomposition of nitrogen dioxide at 383 °C , the rate of the reaction is determined by measuring the appearance of 0,. 2 NO,2 NO + 0, At the beginning of the reaction, the concentration of 0, is O M. After 117 s the concentration has increased to 2.21x102 M. What is the rate of the reaction? (mol 0, /L) / s For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C, the rate of the reaction is determined by measuring the appearance of 0,. 2 H,0,(aq)2 H,0(1) + 0,(g) At the beginning of the reaction, the concentration of O, is O M. After 461 min the concentration has increased to 8.45x10 M. (mol 0,/L) /min What is the rate of the reaction? For the gas phase decomposition of hydrogen peroxide at 400 °C, the rate of the reaction is determined by measuring the disappearance of H,02. 2 H,02-2 H,0 + 0, At the beginning of the reaction, the concentration of H,0, is 0.167 M. After 42.0 s the concentration has dropped to 2.97x102 M. What is the rate of the reaction? (mol H,0,/L) /s

For the gas phase decomposition of nitrogen dioxide at 383 °C , the rate of the reaction is determined by measuring the appearance of 0,. 2 NO,2 NO + 0, At the beginning of the reaction, the concentration of 0, is O M. After 117 s the concentration has increased to 2.21x102 M. What is the rate of the reaction? (mol 0, /L) / s For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C, the rate of the reaction is determined by measuring the appearance of 0,. 2 H,0,(aq)2 H,0(1) + 0,(g) At the beginning of the reaction, the concentration of O, is O M. After 461 min the concentration has increased to 8.45x10 M. (mol 0,/L) /min What is the rate of the reaction? For the gas phase decomposition of hydrogen peroxide at 400 °C, the rate of the reaction is determined by measuring the disappearance of H,02. 2 H,02-2 H,0 + 0, At the beginning of the reaction, the concentration of H,0, is 0.167 M. After 42.0 s the concentration has dropped to 2.97x102 M. What is the rate of the reaction? (mol H,0,/L) /s

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 27QAP: Hydrogen bromide is a highly reactive and corrosive gas used mainly as a catalyst for organic...

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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?
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
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Hydrogen bromide is a highly reactive and corrosive gas used mainly as a catalyst for organic reactions. It is produced by reacting hydrogen and bromine gases together. Â H2(g)+Br2(g)2HBr(g)The rate is followed by measuring the intensity of the orange color of the bromine gas. The following data are obtained: (a) What is the order of the reaction with respect to hydrogen, bromine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. What are the units for k? (d) When [ H2 ]=0.455Mand [ Br2 ]=0.215M, what is the rate of the reaction?
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
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.
Nitrosyl chloride (NOCI) decomposes to nitrogen oxide and chlorine gases. (a) Write a balanced equation using smallest whole-number coefficients for the decomposition. (b) Write an expression for the reaction rate in terms of [NOCl]. (c) The concentration of NOCl drops from 0.580 M to 0.238 M in 8.00 min. Calculate the average rate of reaction over this time interval.
Explain what is meant by the average rate of a reaction.
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?