5.60 L of C2He is completely combusted at 0.500 bar and 313 K according to the reaction below. During the reaction, the pressure and temperature change. In the end, 9.23 L of CO2 are produced and the total pressure of the reaction vessel is 1.56 bar. What is the final temperature of the reaction vessel? (R = 0.08314 L·bar/mol ·K) 2C2H, (g) + 7O2 (g) → 4CO2 (g) + 6H20 (g)
5.60 L of C2He is completely combusted at 0.500 bar and 313 K according to the reaction below. During the reaction, the pressure and temperature change. In the end, 9.23 L of CO2 are produced and the total pressure of the reaction vessel is 1.56 bar. What is the final temperature of the reaction vessel? (R = 0.08314 L·bar/mol ·K) 2C2H, (g) + 7O2 (g) → 4CO2 (g) + 6H20 (g)
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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![**Combustion of Ethane Under Controlled Conditions**
In this experimental setup, 5.60 L of ethane (C₂H₆) is completely combusted at an initial pressure of 0.500 bar and temperature of 313 K. The chemical reaction governing the combustion is:
\[ 2C_2H_6 (g) + 7O_2 (g) \rightarrow 4CO_2 (g) + 6H_2O (g) \]
During the reaction, both the pressure and temperature change. By the end of the reaction, 9.23 L of carbon dioxide (CO₂) is produced, and the total pressure rises to 1.56 bar. The task is to determine the final temperature of the reaction vessel.
**Parameters:**
- Initial volume of C₂H₆: 5.60 L
- Initial pressure: 0.500 bar
- Initial temperature: 313 K
- Final volume of CO₂: 9.23 L
- Final pressure: 1.56 bar
- Gas constant, R: 0.08314 L·bar/mol·K
**Objective:**
Calculate the final temperature of the reaction vessel in Kelvin.
**Procedure:**
1. Apply the ideal gas law and stoichiometry to find the final temperature.
2. Use the relevant gas constant and reaction parameters to solve for temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bd06d49-1f03-4d83-9ba1-5526279a5db3%2Fcfd32b0e-0a8a-4708-8da8-c7500d4d08da%2F98baoe9_processed.png&w=3840&q=75)
Transcribed Image Text:**Combustion of Ethane Under Controlled Conditions**
In this experimental setup, 5.60 L of ethane (C₂H₆) is completely combusted at an initial pressure of 0.500 bar and temperature of 313 K. The chemical reaction governing the combustion is:
\[ 2C_2H_6 (g) + 7O_2 (g) \rightarrow 4CO_2 (g) + 6H_2O (g) \]
During the reaction, both the pressure and temperature change. By the end of the reaction, 9.23 L of carbon dioxide (CO₂) is produced, and the total pressure rises to 1.56 bar. The task is to determine the final temperature of the reaction vessel.
**Parameters:**
- Initial volume of C₂H₆: 5.60 L
- Initial pressure: 0.500 bar
- Initial temperature: 313 K
- Final volume of CO₂: 9.23 L
- Final pressure: 1.56 bar
- Gas constant, R: 0.08314 L·bar/mol·K
**Objective:**
Calculate the final temperature of the reaction vessel in Kelvin.
**Procedure:**
1. Apply the ideal gas law and stoichiometry to find the final temperature.
2. Use the relevant gas constant and reaction parameters to solve for temperature.
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