Study the reaction. H2SO4(1) + CaCO3 (s) = CO2(9) + H2O(1) + Caso4(aq) Which of the following would cause the equilibrium to shift, producing more carbon dioxide gas? Select all that apply. O removing H2 SO4 from the system V removing water from the system V removing carbon dioxide gas from the system V adding CaCO3 to the system
Study the reaction. H2SO4(1) + CaCO3 (s) = CO2(9) + H2O(1) + Caso4(aq) Which of the following would cause the equilibrium to shift, producing more carbon dioxide gas? Select all that apply. O removing H2 SO4 from the system V removing water from the system V removing carbon dioxide gas from the system V adding CaCO3 to the system
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![**Study the Reaction:**
\( \text{H}_2\text{SO}_4(l) + \text{CaCO}_3(s) \rightleftharpoons \text{CO}_2(g) + \text{H}_2\text{O}(l) + \text{CaSO}_4(aq) \)
**Question:**
Which of the following would cause the equilibrium to shift, producing more carbon dioxide gas? Select all that apply.
- [ ] removing \( \text{H}_2\text{SO}_4 \) from the system
- [x] removing water from the system
- [x] removing carbon dioxide gas from the system
- [x] adding \( \text{CaCO}_3 \) to the system
**Explanation:**
To produce more carbon dioxide gas, the following actions will shift the equilibrium position:
1. **Removing Water from the System:** By removing H₂O, we decrease the concentration of products, causing the equilibrium to shift to the right to produce more products, including CO₂.
2. **Removing Carbon Dioxide Gas from the System:** Taking out CO₂ will also shift equilibrium to the right, encouraging the production of more CO₂ to counteract the change.
3. **Adding Calcium Carbonate (CaCO₃):** Increasing the concentration of a reactant typically shifts the equilibrium to the right, promoting the formation of more products, such as CO₂.
The removal of H₂SO₄ from the system would not result in more CO₂, as it would decrease the amount of reactant available.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41677ce8-520f-4674-ac62-3a728523110c%2Fff51d9cf-1148-4f2a-8129-bef391122249%2F30z6msb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Study the Reaction:**
\( \text{H}_2\text{SO}_4(l) + \text{CaCO}_3(s) \rightleftharpoons \text{CO}_2(g) + \text{H}_2\text{O}(l) + \text{CaSO}_4(aq) \)
**Question:**
Which of the following would cause the equilibrium to shift, producing more carbon dioxide gas? Select all that apply.
- [ ] removing \( \text{H}_2\text{SO}_4 \) from the system
- [x] removing water from the system
- [x] removing carbon dioxide gas from the system
- [x] adding \( \text{CaCO}_3 \) to the system
**Explanation:**
To produce more carbon dioxide gas, the following actions will shift the equilibrium position:
1. **Removing Water from the System:** By removing H₂O, we decrease the concentration of products, causing the equilibrium to shift to the right to produce more products, including CO₂.
2. **Removing Carbon Dioxide Gas from the System:** Taking out CO₂ will also shift equilibrium to the right, encouraging the production of more CO₂ to counteract the change.
3. **Adding Calcium Carbonate (CaCO₃):** Increasing the concentration of a reactant typically shifts the equilibrium to the right, promoting the formation of more products, such as CO₂.
The removal of H₂SO₄ from the system would not result in more CO₂, as it would decrease the amount of reactant available.
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