When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3 (s)+CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 55.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3= Submit Part B HA Value Units Butane, C, H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C Ho (9)+1302 (9) 8CO₂ (9)+10H₂O(l) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 1.60 g of butane? Express your answer with the appropriate units. View Available Hint(s)
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3 (s)+CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 55.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3= Submit Part B HA Value Units Butane, C, H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C Ho (9)+1302 (9) 8CO₂ (9)+10H₂O(l) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 1.60 g of butane? Express your answer with the appropriate units. View Available Hint(s)
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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Answer part a and b
![**Educational Content Transcription:**
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**The Ideal Gas Law**
The ideal gas law is represented as:
\[ PV = nRT \]
- **P** represents pressure
- **V** represents volume
- **T** represents temperature
- **n** represents the number of moles of a gas
- **R** is the gas constant, with a value of 0.08206 L·atm/(K·mol) or 8.3145 J/(K·mol)
The equation can be rearranged to solve for moles:
\[ n = \frac{PV}{RT} \]
This equation is useful when dealing with gaseous reactions because stoichiometric calculations often involve mole ratios.
---
**Part A**
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
**Problem:** What is the mass of calcium carbonate needed to produce 55.0 L of carbon dioxide at STP (Standard Temperature and Pressure)?
**Solution:** Express your answer with the appropriate units.
- Mass of CaCO₃ = [Input Field for Value] [Input Field for Units]
**Submit Button**
---
**Part B**
Butane, \( \text{C}_4\text{H}_{10} \), is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is:
\[ 2\text{C}_4\text{H}_{10}(g) + 13\text{O}_2(g) \rightarrow 8\text{CO}_2(g) + 10\text{H}_2\text{O}(l) \]
**Problem:** At 1.10 atm and 23°C, what is the volume of carbon dioxide formed by the combustion of 1.60 g of butane?
**Solution:** Express your answer with the appropriate units.
- Volume of CO₂ = [Input Field for Value] [Input Field for Units]
**Submit Button**
---](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2F6ee011c8-dcb0-4bad-b89a-0578d66e92b6%2Fjuhck7e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content Transcription:**
---
**The Ideal Gas Law**
The ideal gas law is represented as:
\[ PV = nRT \]
- **P** represents pressure
- **V** represents volume
- **T** represents temperature
- **n** represents the number of moles of a gas
- **R** is the gas constant, with a value of 0.08206 L·atm/(K·mol) or 8.3145 J/(K·mol)
The equation can be rearranged to solve for moles:
\[ n = \frac{PV}{RT} \]
This equation is useful when dealing with gaseous reactions because stoichiometric calculations often involve mole ratios.
---
**Part A**
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
**Problem:** What is the mass of calcium carbonate needed to produce 55.0 L of carbon dioxide at STP (Standard Temperature and Pressure)?
**Solution:** Express your answer with the appropriate units.
- Mass of CaCO₃ = [Input Field for Value] [Input Field for Units]
**Submit Button**
---
**Part B**
Butane, \( \text{C}_4\text{H}_{10} \), is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is:
\[ 2\text{C}_4\text{H}_{10}(g) + 13\text{O}_2(g) \rightarrow 8\text{CO}_2(g) + 10\text{H}_2\text{O}(l) \]
**Problem:** At 1.10 atm and 23°C, what is the volume of carbon dioxide formed by the combustion of 1.60 g of butane?
**Solution:** Express your answer with the appropriate units.
- Volume of CO₂ = [Input Field for Value] [Input Field for Units]
**Submit Button**
---
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