4:37Question 11 of 162 NBr3 (g) = N₂ (g) + 3 Br₂ (g)Which of the following changes wouldcause the reaction below to shift in theforward direction to reestablish equilibrium?A) adding a catalyst.B) adding Ar (g).D) adding N₂.5GWC) increasing the total volume of thecontainer.Tap here or pull up for additional resourcesSubmit

Answered: Image /qna-images/answer/67f0936a-4dd4-4fef-a259-edf958b36596.jpg

Which of the following changes would cause the reaction below to shift in the forward direction to reestablish equilibrium? 2 NBr3 (g) = N₂ (g) + 3 Br₂ (g) A) adding a catalyst. B) adding Ar (g). C) increasing the total volume of the container. D) adding N₂.

Which of the following changes would cause the reaction below to shift in the forward direction to reestablish equilibrium? 2 NBr3 (g) = N₂ (g) + 3 Br₂ (g) A) adding a catalyst. B) adding Ar (g). C) increasing the total volume of the container. D) adding N₂.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 1QAP: The following data are for the system A(g)2B(g) (a) How long does it take the system to reach...

See similar textbooks

Similar questions

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?
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.
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 student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
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.
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.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
The figures below represent the following reaction at equilibrium at different temperatures. A2(g)+3B2(g)2AB3(g)where squares represent atom A and circles represent atom B. Is the reaction exothermic?
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.