Consider the following system2 NO(g) + Br2 (9)at equilibrium at 298 K.2 NOBr(g)Use the References to access inWhen some Br₂ (g) is added to the equilibrium system at constant temperature, the reaction mustO run in the forward direction to reestablish equilibrium.O run in the reverse direction to reestablish equilibrium.O remain the same. It is already at equilibrium.The concentration of NO willO increase.O decrease.O remain the same.

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Use the References to access Consider the following system 2 NO(g) + Br2 (9) When some Br2 (g) is added to the equilibrium system at constant temperature, the reaction mus O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The concentration of NO will O increase. O decrease. O remain the same. at equilibrium at 298 K. 2 NOBr(g)

Use the References to access Consider the following system 2 NO(g) + Br2 (9) When some Br2 (g) is added to the equilibrium system at constant temperature, the reaction mus O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The concentration of NO will O increase. O decrease. O remain the same. at equilibrium at 298 K. 2 NOBr(g)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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Similar questions

5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?
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.