What volume of carbon dioxide is produced when 16.1 g of calcium carbonate reacts completely according to the follo reaction at 25 °C and 1 atm? calcium carbonate (s) calcium oxide (s) + carbon dioxide(g) liters carbon dioxide
What volume of carbon dioxide is produced when 16.1 g of calcium carbonate reacts completely according to the follo reaction at 25 °C and 1 atm? calcium carbonate (s) calcium oxide (s) + carbon dioxide(g) liters carbon dioxide
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...
Related questions
Question
![### Chemical Reaction and Carbon Dioxide Volume Calculation
#### Problem Statement
What volume of carbon dioxide is produced when 16.1 g of calcium carbonate reacts completely according to the following reaction at 25°C and 1 atm?
#### Chemical Reaction
\[ \text{calcium carbonate (s)} \rightarrow \text{calcium oxide (s)} + \text{carbon dioxide(g)} \]
#### Data Input
* Mass of calcium carbonate: 16.1 g
* Temperature: 25°C
* Pressure: 1 atm
#### Data Required
* Volume of carbon dioxide produced (in liters)
#### Procedure
1. **Identify the molar mass of calcium carbonate (CaCO₃)**:
- Calcium (Ca): 40.08 g/mol
- Carbon (C): 12.01 g/mol
- Oxygen (O): 16.00 g/mol (x 3)
- Molar mass of CaCO₃ = 40.08 + 12.01 + (16.00 x 3) = 100.09 g/mol
2. **Calculate the moles of calcium carbonate**:
\[
\text{Moles of CaCO₃} = \frac{\text{mass of CaCO₃}}{\text{molar mass of CaCO₃}} = \frac{16.1\ g}{100.09\ g/mol}
\]
3. **Use the stoichiometry of the reaction**:
- The reaction shows a 1:1 molar ratio between CaCO₃ and CO₂.
- Therefore, moles of CaCO₃ will equal moles of CO₂ produced.
4. **Calculate the volume of CO₂ produced**:
- Use the Ideal Gas Law: PV = nRT
- Where:
- P is the pressure (1 atm),
- V is the volume,
- n is the number of moles,
- R is the gas constant (0.0821 L atm / K mol),
- T is the temperature in Kelvin (25°C + 273.15 = 298.15 K).
\[
V = \frac{nRT}{P} = \frac{(\text{moles of CO₂}) \cdot (0.0821\ L\ atm / K\ mol) \cdot (298.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60358686-21d1-41ff-a93a-9ba59c7b6516%2F1ddd1e70-c5e8-4bff-b6af-e6513a43ab60%2F73r33i_reoriented.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction and Carbon Dioxide Volume Calculation
#### Problem Statement
What volume of carbon dioxide is produced when 16.1 g of calcium carbonate reacts completely according to the following reaction at 25°C and 1 atm?
#### Chemical Reaction
\[ \text{calcium carbonate (s)} \rightarrow \text{calcium oxide (s)} + \text{carbon dioxide(g)} \]
#### Data Input
* Mass of calcium carbonate: 16.1 g
* Temperature: 25°C
* Pressure: 1 atm
#### Data Required
* Volume of carbon dioxide produced (in liters)
#### Procedure
1. **Identify the molar mass of calcium carbonate (CaCO₃)**:
- Calcium (Ca): 40.08 g/mol
- Carbon (C): 12.01 g/mol
- Oxygen (O): 16.00 g/mol (x 3)
- Molar mass of CaCO₃ = 40.08 + 12.01 + (16.00 x 3) = 100.09 g/mol
2. **Calculate the moles of calcium carbonate**:
\[
\text{Moles of CaCO₃} = \frac{\text{mass of CaCO₃}}{\text{molar mass of CaCO₃}} = \frac{16.1\ g}{100.09\ g/mol}
\]
3. **Use the stoichiometry of the reaction**:
- The reaction shows a 1:1 molar ratio between CaCO₃ and CO₂.
- Therefore, moles of CaCO₃ will equal moles of CO₂ produced.
4. **Calculate the volume of CO₂ produced**:
- Use the Ideal Gas Law: PV = nRT
- Where:
- P is the pressure (1 atm),
- V is the volume,
- n is the number of moles,
- R is the gas constant (0.0821 L atm / K mol),
- T is the temperature in Kelvin (25°C + 273.15 = 298.15 K).
\[
V = \frac{nRT}{P} = \frac{(\text{moles of CO₂}) \cdot (0.0821\ L\ atm / K\ mol) \cdot (298.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 4 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY