The equilibrium constant, Ke, for the following reaction is 0.00650 at 298 K.2NOBr(g) 2NO(g) + Br₂ (g)$4Forms Office of t... KB Viewing Your Aca...Submit AnswerIf an equilibrium mixture of the three gases in a 17.8 L container at 298 K contains 0.378 mol of NOBr(g) and 0.461mol of NO, the equilibrium concentration of Br₂ IsM.000000 F4RFShow Hint%5Scholarship Ameri...[Review Topics][References]Use the References to access important values if needed for this question.Retry Entire Group 9 more group attempts remainingTGCengage Learning Cengage Technical Support^6Have Changes in...MacBook AirSYH&7F7U*8►IIF8(9KAF9O-0)bio 1108 chatF10SAVAGE X FENTY...PreviousF11+11Next>Save and ExitF1217

Answered: Image /qna-images/answer/f85def1e-6b8d-4164-a36e-e995c515fe40.jpg

Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 0.00650 at 298 K. 2NOBr(g)2NO(g) + Br₂ (9) If an equilibrium mixture of the three gases in a 17.8 L container at 298 K contains 0.378 mol of NOBr(g) and 0.461 mol of NO, the equilibrium concentration of Br2 Is M. Submit Answer Retry Entire Group 9 more group attempts remaining

Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 0.00650 at 298 K. 2NOBr(g)2NO(g) + Br₂ (9) If an equilibrium mixture of the three gases in a 17.8 L container at 298 K contains 0.378 mol of NOBr(g) and 0.461 mol of NO, the equilibrium concentration of Br2 Is M. Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ: Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105...

See similar textbooks

Similar questions

For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
Consider the following statements: Consider the reaction A(g)+B(g)C(g),for which at equilibrium [A] = 2 M, [B] = 1 M, and [C] = 4 M. To a 1-L container of the system at equilibrium, you add 3 moles of B. A possible equilibrium condition is [A] = 1 M, [B] = 3 M, and [C] = 6 M because in both cases K = 2. Indicate everything that is correct in these statements and everything that is incorrect. Correct the incorrect statements, and explain.
Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g)C2H6CO(g)+H2(g)At 180C, the equilibrium constant for the decomposition is 0.45. If 20.0 mL (d=0.785g/mL) of isopropyl alcohol is placed in a 5.00-L vessel and heated to 180C, what percent- age remains undissociated at equilibrium?
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
A 1.00-L vessel at 400 C contains the following equilibrium concentrations: N2, 1.00 M; H2, 0.50 M; and NH3, 0.25 M. How many moles of hydrogen must be removed from the vessel to increase the concentration of nitrogen to 1.1 M?
Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium mixture in a 5.00-L flask at 443 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?
Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 45 s? After 90 s?
Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, bow many molecules of H2O, CO, H2, and CO2 are present? Do this problem by trial and error-that is, if two molecules of CO react, is this equilibrium; if three molecules of CO react, is this equilibrium; and so on.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.