Consider this reaction: 2H2S(e + 302(g) <----> 2H20 + 2S02(2) H=-1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium when the equilibrium is disturbed by a) expanding the container b) removing SO2
Consider this reaction: 2H2S(e + 302(g) <----> 2H20 + 2S02(2) H=-1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium when the equilibrium is disturbed by a) expanding the container b) removing SO2
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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Please answer a and b
![### Reaction Equilibrium Analysis
Consider the following reaction:
\[ 2\text{H}_2\text{S}_{(g)} + 3\text{O}_2_{(g)} \rightleftharpoons 2\text{H}_2\text{O}_{(g)} + 2\text{SO}_2_{(g)} \quad \Delta H = -1036 \, \text{kJ} \]
Predict whether the forward or reverse reaction will re-establish equilibrium when the equilibrium is disturbed by:
a) Expanding the container
b) Removing \(\text{SO}_2\)
c) Raising the temperature
d) Water vapor is added
### Graphs and Diagrams
There are no graphs or diagrams associated with this text.
---
In this reaction, the equilibrium can be influenced by changes in volume, concentration of reactants or products, temperature, and the addition of other substances. Understanding how these factors affect the reaction can help predict whether the forward or reverse reaction will dominate to re-establish equilibrium in response to the disturbance.
For more details, refer to the principles of Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any changes imposed upon it, thus re-establishing equilibrium.
### Detailed Analysis
#### a) Expanding the container
Expanding the container decreases the pressure of the system. For reactions involving gases, the system will shift toward the side with more moles of gas to counteract this change. For this reaction:
\[ \text{Reactants: } (2 + 3) = 5 \text{ moles of gas} \]
\[ \text{Products: } 2 + 2 = 4 \text{ moles of gas} \]
Since there are more moles of gas on the reactants' side, the equilibrium will shift towards the reactants (reverse reaction).
#### b) Removing \(\text{SO}_2\)
Removing \(\text{SO}_2\) decreases the concentration of one of the products. To counteract this change, the equilibrium will shift towards the products (forward reaction) to increase the concentration of \(\text{SO}_2\).
#### c) Raising the temperature
This reaction is exothermic (\(\Delta H = -1036 \, \text{kJ}\)). Increasing the temperature will add heat to the system. According to Le](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa948129d-0f95-4d62-b5fb-72551c83c8d3%2F917f1446-9359-4e35-8049-ef6f3e8cfad4%2F1cpu4d7h_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction Equilibrium Analysis
Consider the following reaction:
\[ 2\text{H}_2\text{S}_{(g)} + 3\text{O}_2_{(g)} \rightleftharpoons 2\text{H}_2\text{O}_{(g)} + 2\text{SO}_2_{(g)} \quad \Delta H = -1036 \, \text{kJ} \]
Predict whether the forward or reverse reaction will re-establish equilibrium when the equilibrium is disturbed by:
a) Expanding the container
b) Removing \(\text{SO}_2\)
c) Raising the temperature
d) Water vapor is added
### Graphs and Diagrams
There are no graphs or diagrams associated with this text.
---
In this reaction, the equilibrium can be influenced by changes in volume, concentration of reactants or products, temperature, and the addition of other substances. Understanding how these factors affect the reaction can help predict whether the forward or reverse reaction will dominate to re-establish equilibrium in response to the disturbance.
For more details, refer to the principles of Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any changes imposed upon it, thus re-establishing equilibrium.
### Detailed Analysis
#### a) Expanding the container
Expanding the container decreases the pressure of the system. For reactions involving gases, the system will shift toward the side with more moles of gas to counteract this change. For this reaction:
\[ \text{Reactants: } (2 + 3) = 5 \text{ moles of gas} \]
\[ \text{Products: } 2 + 2 = 4 \text{ moles of gas} \]
Since there are more moles of gas on the reactants' side, the equilibrium will shift towards the reactants (reverse reaction).
#### b) Removing \(\text{SO}_2\)
Removing \(\text{SO}_2\) decreases the concentration of one of the products. To counteract this change, the equilibrium will shift towards the products (forward reaction) to increase the concentration of \(\text{SO}_2\).
#### c) Raising the temperature
This reaction is exothermic (\(\Delta H = -1036 \, \text{kJ}\)). Increasing the temperature will add heat to the system. According to Le
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