Two moles of a sample of an ideal gas at 25⁰C is allowed to expand reversibly and isothermally from 1 dm³ to 10 dm³. What is ΔS, for the gas, and what is ΔS for its surroundings? b. The same gas is expanded adiabatically and irreversibly from 1 dm³ to 10 dm³ with no work done. What is the final temperature of the gas? What is ΔS for the gas and ΔS for the surroundings? What is the ΔS(tot)?
Two moles of a sample of an ideal gas at 25⁰C is allowed to expand reversibly and isothermally from 1 dm³ to 10 dm³. What is ΔS, for the gas, and what is ΔS for its surroundings? b. The same gas is expanded adiabatically and irreversibly from 1 dm³ to 10 dm³ with no work done. What is the final temperature of the gas? What is ΔS for the gas and ΔS for the surroundings? What is the ΔS(tot)?
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter2: The First Law Of Thermodynamics
Section: Chapter Questions
Problem 2.24E: Calculate the work donewhen 1.000 mole of an ideal gas expands reversiblyfrom 1.0L to 10L at 298.0K....
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Two moles of a sample of an ideal gas at 25⁰C is allowed to expand reversibly and isothermally from 1 dm³ to 10 dm³.
What is ΔS, for the gas, and what is ΔS for its surroundings? b. The same gas is expanded adiabatically and irreversibly from 1 dm³ to 10 dm³ with no work done.
What is the final temperature of the gas?
What is ΔS for the gas and ΔS for the surroundings?
What is the ΔS(tot)?
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