Part CConsider the reaction5Br(aq) + BrO (aq) + 6H+ (aq) →3Br2 (aq) + 3H₂O(1)The average rate of consumption of Br is 1.56x10-4 M/s over the first two minutes. What is the average rate of formation of Br₂ during the same time interval?Express your answer with the appropriate units.► View Available Hint(s)μÅRate of formation of Br₂ = ValueSubmitUnits? Part AConsider the reactionUsing the information in the following table, calculate the average rate of formation of P₂O5 between 10.0 and 40.0 s.10.00Express your answer with the appropriate units.► View Available Hint(s)μARate of formation of P₂O5 = ValueSubmitUnits2H3PO4 →P2O5 + 3H₂O?20.030.040.050.0Time (s)[P2O5] (M) 01.10x10-3 4.10x10-3 5.90x10-3 7.10x10-³ 7.70x10-3

Part C Consider the reaction 5Br (aq) + BrO (aq) + 6H+ (aq) →3Br2 (aq) + 3H₂O(1) The average rate of consumption of Br is 1.56x10-4 M/s over the first two minutes. What is the average rate of formation of Br₂ during the same time interval? Express your answer with the appropriate units. ► View Available Hint(s) μÅ Rate of formation of Br₂ = Value Submit Units ?

Part C Consider the reaction 5Br (aq) + BrO (aq) + 6H+ (aq) →3Br2 (aq) + 3H₂O(1) The average rate of consumption of Br is 1.56x10-4 M/s over the first two minutes. What is the average rate of formation of Br₂ during the same time interval? Express your answer with the appropriate units. ► View Available Hint(s) μÅ Rate of formation of Br₂ = Value Submit Units ?

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 30QAP

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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?
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?
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.
Hydrogen peroxide (H20i) decomposes into water and oxygen: H,O2(aq) — H,O(f) + ^O2(g) Ordinarily this reaction proceeds rather slowly, hut in the presence of some iodide ions (I-), the decomposition is much faster. Ihe decomposition in the presence of iodide was studied at 20°C, and the data were plotted in various ways. Use the graphs below to answer the questions that follow. What is the order of reaction for the decomposition of hydrogen peroxide? Find the numerical value of the rate constant at 20°C, including the correct units. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t = 0 in the graphs).
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. SO2Cl2(g)SO2(g)+Cl2(g)At a certain temperature, the half-life of SO2Cl2 is 7.5102 min. Consider a sealed flask with 122.0 g of SO2Cl2. (a) How long will it take to reduce the amount of SO2Cl2 in the sealed flask to 45.0 g? (b) If the decomposition is stopped after 29.0 h, what volume of Cl2 at 27C and 1.00 atm is produced?
Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2NO(g)+2H2(g)N2(g)+2H2O(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration [NO] (mol/L) Initial Concentration, [H2] (mol/L) Initial Rate of Formation of N2 (mol/L min) 1 0.0060 0.0010 1.8104 2 0.0060 0.0020 3.6104 3 0.0010 0.0060 0.30104 4 0.0020 0.0060 1.2104 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO+NON2O2 Step 2: N2O2+H2H2O+N2O Step 3: N2O+H2N2+H2O Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction.
Consider the following hypothetical reaction: X( g )Y( g ) A 200.0-mL flask is filled with 0.120 moles of X. The disappearance of X 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 appearance of Y. (b) Calculate the average disappearance of X in M/S in the first two 20-minute intervals. (c) What is the average rate of appearance of Y between the 20- and 60-minute intervals?
In the PhET Reactions tab to observe how multiple atoms and molecules interact under varying conditions. Select a molecule to pump into the chamber. Set the initial temperature and select the current amounts of each reactant. Select Show bonds under Options. How is the rate of the reaction affected by concentration and temperature?
When nitrogen dioxide reacts with carbon monoxide, the following reaction occurs. Â NO2(g)+CO(g)NO(g)+CO2(g)The following data are obtained at a certain temperature: (a) What is the order of the reaction with respect to NO2, CO, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) When [ NO2 ]=0.421Mand [ CO ]=0.816M, what is the rate of the reaction at the temperature of the experiments?