### Chemical Equilibrium and Volume Changes**Consider the following system at equilibrium at 350 K:**\[ \text{CH}_4(g) + \text{CCl}_4(g) \rightleftharpoons 2 \text{CH}_2\text{Cl}_2(g) \]**If the VOLUME of the equilibrium system is suddenly increased at constant temperature:****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.**The number of moles of \(\text{CCl}_4\) will:**- ( ) A. Increase.- ( ) B. Decrease.- ( ) C. Remain the same.### Analysis:#### Understanding the System:- At 350 K, the system is in equilibrium.- The reaction involves methane (\(\text{CH}_4\)) and carbon tetrachloride (\(\text{CCl}_4\)) reacting to form dichloromethane (\(\text{CH}_2\text{Cl}_2\)).- Initially, all gases are in balance.#### Effect of Volume Increase:- When the volume is increased, the pressure of the system decreases.- According to Le Chatelier's Principle, the system will adjust to counteract this change by shifting the equilibrium.#### Reaction Shift:- Here, the forward reaction produces more molecules: from 2 moles of reactants to 2 moles of products.- Since the number of gas molecules remains the same (2 to 2), changing the volume will not necessarily shift the equilibrium towards more or fewer moles, as the total number of moles of gases remains consistent.Thus, the correct choices are:1. **The reaction must:** - ( ) C. Remain the same. Already at equilibrium.2. **The number of moles of \(\text{CCl}_4\) will:** - ( ) C. Remain the same.In scenarios involving changes in volume, it’s crucial to understand the overall effect on molecule count and gas pressure's impact on equilibrium.

According to Le Chatelier's principle, the reaction shifts in the direction where we have less…

Consider the following system at equilibrium at 350 K: CHĄ(g) + CC4(g) =2CH,C2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: A. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The number of moles of CCl4 will: |A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium at 350 K: CHĄ(g) + CC4(g) =2CH,C2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: A. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The number of moles of CCl4 will: |A. Increase. B. Decrease. C. Remain the same.

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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