Hi cyclonextreme. Welcome to Physics Forums.Cyclonextreme said:Homework Statement
A 1.00 mol sample of an ideal diatomic gas, originally at 1 atm and 20°C, expands adiabatically to 2.0 times its initial volume. (Assume no molecular vibration.)
What is the final pressure for the gas?
What is the final temperature for the gas?
(it should be near 40 Celcius)
I can't find anything relatable besides PV=nRT and something with 5/3?
Chestermiller said:Hi cyclonextreme. Welcome to Physics Forums.
Do you know the equations for adiabatic reversible expansion? If not, look them up in your textbook. Study the section on reversible adiabatic expansion.
An ideal diatomic gas is a theoretical model of a gas that consists of particles with no size or volume, and whose interactions are negligible. It follows the ideal gas law, which states that the pressure, volume, and temperature of a gas are directly proportional.
The final temperature of an ideal diatomic gas can be calculated using the ideal gas law, which states that the product of the pressure and volume of a gas is directly proportional to its temperature. Therefore, the final temperature will depend on the initial temperature, pressure, and volume of the gas.
The final pressure of an ideal diatomic gas can also be calculated using the ideal gas law. As the pressure and volume of an ideal gas are directly proportional to its temperature, the final pressure will depend on the initial pressure, volume, and temperature of the gas.
The final temperature and pressure of an ideal diatomic gas can be calculated using the ideal gas law, which states that PV=nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. By manipulating this equation, the final temperature and pressure can be determined.
The ideal diatomic gas model is a theoretical model and differs from real gases in that it assumes the particles have no size or volume and do not interact with each other. In reality, gases do have a finite volume and do interact with each other, although these effects may be negligible under certain conditions.