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A 2.00-mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of and a volume of to a final volume of . What are the initial and final temperatures?
Solution
VerifiedConcepts and Principles
- When an ideal gas undergoes a slow adiabatic volume change (), its pressure and volume are related by:
Where is the ratio of molar specific heats for the gas. For a diatomic gas, .
- Equation of State of an Ideal Gas: an ideal gas is one for which the pressure , volume , and temperature are related by:
Where,
is the number of moles of the gas present.
is the universal gas constant and has a value .
- The change in the internal energy of moles of a confined ideal gas that undergoes a temperature change due to any process is:
Where is the molar specific heat at constant volume for the gas.
- First Law of Thermodynamics: it is the principle of conservation of energy for a thermodynamic process which is expressed as:
Where is the internal energy of the system, is the energy transferred into the system by heat between the system and its surroundings, and is the work done on the system.
In this problem, I am displaying rounded intermediate values for practical purposes. However, calculations are made using the unrounded values.
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