Look at the reaction below and state which direction the reaction would shift: A closed container of water and its vapor at equilibrium. Vapor is added to the system. Water + Energy <=> Vapor
Look at the reaction below and state which direction the reaction would shift: A closed container of water and its vapor at equilibrium. Vapor is added to the system. Water + Energy <=> Vapor
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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Explain why it would shift that certain way
![**Equilibrium Reaction Shift Analysis**
**Scenario:**
Consider the following reaction and determine the direction in which the reaction would shift:
In a closed container of water and its vapor at equilibrium, additional vapor is added to the system.
**Chemical Equation:**
\[ \text{Water + Energy} \rightleftharpoons \text{Vapor} \]
**Explanation:**
According to Le Chatelier’s principle, if a change is imposed on a system at equilibrium, the system will adjust to counteract that change and re-establish equilibrium. In this scenario, adding vapor to the system causes an increase in vapor concentration. To offset this, the reaction will shift towards the left, favoring the formation of liquid water, thereby consuming some of the added vapor.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41677ce8-520f-4674-ac62-3a728523110c%2F970f59ad-9c50-4001-8acf-4c03db424cbb%2Fniy2cet_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium Reaction Shift Analysis**
**Scenario:**
Consider the following reaction and determine the direction in which the reaction would shift:
In a closed container of water and its vapor at equilibrium, additional vapor is added to the system.
**Chemical Equation:**
\[ \text{Water + Energy} \rightleftharpoons \text{Vapor} \]
**Explanation:**
According to Le Chatelier’s principle, if a change is imposed on a system at equilibrium, the system will adjust to counteract that change and re-establish equilibrium. In this scenario, adding vapor to the system causes an increase in vapor concentration. To offset this, the reaction will shift towards the left, favoring the formation of liquid water, thereby consuming some of the added vapor.
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