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Consider the following system at equilibrium where AH° = -87.9 kJ, and K. 83.3, at 500 K: %3D PCI3 (g) + Cl2 (g) =PCI3 (g) If the TEMPERATURE on the equilibrium system is suddenly increased The value of K. A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than K. B. Is equal to K. C. Is less than K. 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 concentration of Cl, will: A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium where AH° = -87.9 kJ, and K. 83.3, at 500 K: %3D PCI3 (g) + Cl2 (g) =PCI3 (g) If the TEMPERATURE on the equilibrium system is suddenly increased The value of K. A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than K. B. Is equal to K. C. Is less than K. 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 concentration of Cl, will: A. Increase. B. Decrease. C. Remain the same.

Chemistry
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 where ΔHº = -87.9 kJ, and Kc = 83.3, at 500 K: \[ \text{PCl}_3 \, (g) + \text{Cl}_2 \, (g) \rightleftharpoons \text{PCl}_5 \, (g) \] If the **TEMPERATURE** on the equilibrium system is suddenly increased: 1. The value of **Kc:** - A. Increases - B. Decreases - C. Remains the same 2. The value of **Qc:** - A. Is greater than **Kc** - B. Is equal to **Kc** - C. Is less than **Kc** 3. The reaction must: - A. Run in the forward direction to reestablish equilibrium. - B. Run in the reverse direction to reestablish equilibrium. - C. Remain the same. Already at equilibrium. 4. The concentration of **Cl2** will: - A. Increase - B. Decrease - C. Remain the same Feedback options include "Submit Answer," "Retry Entire Group," and a note indicating "8 more group attempts remaining."
Transcribed Image Text:Consider the following system at equilibrium where ΔHº = -87.9 kJ, and Kc = 83.3, at 500 K: \[ \text{PCl}_3 \, (g) + \text{Cl}_2 \, (g) \rightleftharpoons \text{PCl}_5 \, (g) \] If the **TEMPERATURE** on the equilibrium system is suddenly increased: 1. The value of **Kc:** - A. Increases - B. Decreases - C. Remains the same 2. The value of **Qc:** - A. Is greater than **Kc** - B. Is equal to **Kc** - C. Is less than **Kc** 3. The reaction must: - A. Run in the forward direction to reestablish equilibrium. - B. Run in the reverse direction to reestablish equilibrium. - C. Remain the same. Already at equilibrium. 4. The concentration of **Cl2** will: - A. Increase - B. Decrease - C. Remain the same Feedback options include "Submit Answer," "Retry Entire Group," and a note indicating "8 more group attempts remaining."
Expert Solution
Introduction

The direction in which a reaction occurs, depends on several factors. The factors are temperature, moles of reactants and products, pressure, and volume. The direction of the reaction is determined by using the Le-chatlier’s principle.

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