The exothermic process C6H1206(s) + 602(g) = 6CO2(g) + 6H20(g) is initially at equilibrium. Which of the following statements is/are true? (Select all that apply.)
The exothermic process C6H1206(s) + 602(g) = 6CO2(g) + 6H20(g) is initially at equilibrium. Which of the following statements is/are true? (Select all that apply.)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 121QRT: When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above...
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![**Equilibrium Reactions in Exothermic Processes**
The exothermic process described by the chemical equation:
\[ \text{C}_6\text{H}_{12}\text{O}_6(\text{s}) + 6\text{O}_2(\text{g}) \leftrightarrow 6\text{CO}_2(\text{g}) + 6\text{H}_2\text{O}(\text{g}) \]
is initially at equilibrium. The following statements pertain to the effects of various changes on this equilibrium:
1. **Adding CO₂(g) causes K to increase.**
- K, the equilibrium constant, is determined only by temperature and is independent of the concentrations of reactants or products. Therefore, adding CO₂ does not cause K to increase, making this statement **false**.
2. **Decreasing the volume causes the reaction to shift left.**
- Decreasing the volume increases the pressure. According to Le Chatelier's Principle, the reaction will shift to the side with fewer moles of gas to reduce pressure. Here, there are 6 moles of gases on both sides, so changing the volume will not shift the equilibrium. Thus, this statement is **false**.
3. **Increasing the temperature causes the reaction to shift right.**
- For an exothermic reaction, increasing the temperature adds heat, which shifts the equilibrium to the left (towards the reactants) to counteract the added heat. Therefore, this statement is **false**.
4. **Adding C₆H₁₂O₆(s) causes Q to decrease.**
- Q, the reaction quotient, is calculated using the concentrations of the gaseous reactants and products. Since C₆H₁₂O₆ is a solid, adding it does not affect Q. Consequently, this statement is **false**.
5. **Adding O₂(g) causes the reaction to shift right.**
- According to Le Chatelier's Principle, adding more of a reactant (O₂) will shift the equilibrium to the right (towards the products) to counteract the change. Thus, this statement is **true**.
By selecting the statements that are true based on the principles of chemical equilibrium, the correct answer would be:
\- Adding O₂(g) causes the reaction to shift right.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdb8ba6cb-f074-43c1-b7bc-05cc004f9981%2F0382819a-ba41-44cd-8fc8-b044882d5804%2Fg95k3x_processed.png&w=3840&q=75)
Transcribed Image Text:**Equilibrium Reactions in Exothermic Processes**
The exothermic process described by the chemical equation:
\[ \text{C}_6\text{H}_{12}\text{O}_6(\text{s}) + 6\text{O}_2(\text{g}) \leftrightarrow 6\text{CO}_2(\text{g}) + 6\text{H}_2\text{O}(\text{g}) \]
is initially at equilibrium. The following statements pertain to the effects of various changes on this equilibrium:
1. **Adding CO₂(g) causes K to increase.**
- K, the equilibrium constant, is determined only by temperature and is independent of the concentrations of reactants or products. Therefore, adding CO₂ does not cause K to increase, making this statement **false**.
2. **Decreasing the volume causes the reaction to shift left.**
- Decreasing the volume increases the pressure. According to Le Chatelier's Principle, the reaction will shift to the side with fewer moles of gas to reduce pressure. Here, there are 6 moles of gases on both sides, so changing the volume will not shift the equilibrium. Thus, this statement is **false**.
3. **Increasing the temperature causes the reaction to shift right.**
- For an exothermic reaction, increasing the temperature adds heat, which shifts the equilibrium to the left (towards the reactants) to counteract the added heat. Therefore, this statement is **false**.
4. **Adding C₆H₁₂O₆(s) causes Q to decrease.**
- Q, the reaction quotient, is calculated using the concentrations of the gaseous reactants and products. Since C₆H₁₂O₆ is a solid, adding it does not affect Q. Consequently, this statement is **false**.
5. **Adding O₂(g) causes the reaction to shift right.**
- According to Le Chatelier's Principle, adding more of a reactant (O₂) will shift the equilibrium to the right (towards the products) to counteract the change. Thus, this statement is **true**.
By selecting the statements that are true based on the principles of chemical equilibrium, the correct answer would be:
\- Adding O₂(g) causes the reaction to shift right.
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