**Chemical Equilibrium and Le Chatelier's Principle****Question:**Consider the following reaction carried out at constant temperature and volume.\[ \text{Cl}_2(g) + \text{H}_2(g) \rightleftharpoons 2\text{HCl}(g) \]What is the effect of removing some HCl from the system at equilibrium?**Options:**- \( \circ \) The \( \text{Cl}_2 \) and \( \text{H}_2 \) concentrations decrease equally.- \( \circ \) The \( \text{H}_2 \) concentration decreases more than the \( \text{Cl}_2 \) concentration.- \( \circ \) The \( \text{Cl}_2 \) and \( \text{H}_2 \) concentrations remain the same.- \( \circ \) The \( \text{Cl}_2 \) concentration decreases more than the \( \text{H}_2 \) concentration.**Graph/Diagram Explanation:**No graphs or diagrams are included in the original question. The question focuses on understanding the qualitative changes in concentration of reactants and products when one product (\(\text{HCl}\)) is removed from the equilibrium system.**Understanding the Concept:**Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust itself in such a way as to counteract that disturbance and restore a new equilibrium. In this question, when some \(\text{HCl}(g)\) is removed, the equilibrium will shift to the right to produce more \(\text{HCl}(g)\) by consuming more \(\text{Cl}_2(g)\) and \(\text{H}_2(g)\).**Follow-Up:**These options and the underlying principle provide students with a clear understanding of how equilibrium systems respond to changes, specifically focusing on the removal of a product from the reaction mixture.

Consider the following reaction carried out at constant temperature and volume. Cl, (g) + H,(g) = 2HCI(g) What is the effect of removing some HCI from the system at equilibrium? The Cl, and H, concentrations decrease equally. The H, concentration decreases more than the Cl, concentration. The Cl, and H, concentrations remain the same. The Cl, concentration decreases more than the H, concentration.

Consider the following reaction carried out at constant temperature and volume. Cl, (g) + H,(g) = 2HCI(g) What is the effect of removing some HCI from the system at equilibrium? The Cl, and H, concentrations decrease equally. The H, concentration decreases more than the Cl, concentration. The Cl, and H, concentrations remain the same. The Cl, concentration decreases more than the H, concentration.

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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