Consider the following system at equilibrium at 600 K:COCl2 (g) CO (g) + Cl2 (g)If the PRESSURE of the equilibrium system is suddenly decreased at constant temperature:The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium.The number of moles of Cl2 will: A. Increase. B. Decrease. C. Remain the same.Consider the following system at equilibrium at 800 K:2H2(g) + S2(g) 2H2S(g)If the PRESSURE of the equilibrium system is suddenly decreased at constant temperature:The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium.The number of moles of S2 will: A. Increase. B. Decrease. C. Remain the same.Consider the following system at equilibrium at 600 K:COCl2 (g) + 25.9 kcal CO (g) + Cl2 (g)Indicate whether each individual change would favor the production of CO (g). Evaluate each change separately, assuming that all other conditions remain constant. Increasing the temperature. Increasing the pressure. Increasing the volume. Removing COCl2 . Adding Cl2 . Consider the following system at equilibrium at 800 K:2H2(g) + S2(g) 2H2S(g) + 69.3 kcalIndicate whether each individual change would favor the production of H2S(g). Evaluate each change separately, assuming that all other conditions remain constant. Increasing the temperature. Decreasing the pressure. Increasing the volume. Adding H2S. Removing S2.

When the reaction is in equilibrium then the any change drives the reaction in such a way that the…

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following system at equilibrium at 600 K:

COCl₂ (g) CO (g) + Cl₂ (g)

If the PRESSURE of the equilibrium system is suddenly decreased at constant temperature:

The reaction must:		A. Run in the forward direction to restablish equilibrium.
		B. Run in the reverse direction to restablish equilibrium.
		C. Remain the same. Already at equilibrium.

The number of moles of Cl₂ will:		A. Increase.
		B. Decrease.
		C. Remain the same.

Consider the following system at equilibrium at 800 K:

2H₂(g) + S₂(g) 2H₂S(g)

If the PRESSURE of the equilibrium system is suddenly decreased at constant temperature:

The reaction must:		A. Run in the forward direction to restablish equilibrium.
		B. Run in the reverse direction to restablish equilibrium.
		C. Remain the same. Already at equilibrium.

The number of moles of S₂ will:		A. Increase.
		B. Decrease.
		C. Remain the same.

Consider the following system at equilibrium at 600 K:

COCl₂ (g) + 25.9 kcal CO (g) + Cl₂ (g)

Indicate whether each individual change would favor the production of CO (g). Evaluate each change separately, assuming that all other conditions remain constant.

Increasing the temperature.
Increasing the pressure.
Increasing the volume.
Removing COCl₂ .
Adding Cl₂ .

Consider the following system at equilibrium at 800 K:

2H₂(g) + S₂(g) 2H₂S(g) + 69.3 kcal

Indicate whether each individual change would favor the production of H₂S(g). Evaluate each change separately, assuming that all other conditions remain constant.

Increasing the temperature.
Decreasing the pressure.
Increasing the volume.
Adding H₂S.
Removing S₂.

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