What is the final pressure of an adiabatically compressed gas in a container?

In summary, the question involves a container with air being compressed adiabatically from an initial volume of 2.0 L at a pressure of 1.0 atm and temperature of -50C, to a final volume of 0.5 L. The final pressure is unknown and cannot be determined using the ideal gas law due to the adiabatic process. The solution may involve finding the number of moles, but this is not given in the problem.
  • #1
de3tz
1
0

Homework Statement


a container with air (M = 29 g/mol, treated as an ideal gas). In the container, we have 2.0 L of the gas with p1 = 1.0 atm at T1 = – 50C. The gas is compressed adiabatically to a final volume of 0.5 L. What is its final pressure?


Homework Equations


I am really not sure, as the moles are not given, and the only equation I have encountered for this problem involves moles.


The Attempt at a Solution


I attempted using ideal gas law, but since the process is adiabatic, the answer does not apply. I am truly confused.
 
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  • #2
Do you think you could find moles? I mean, you have Pressure, Volume, and Temperature.
 

FAQ: What is the final pressure of an adiabatically compressed gas in a container?

What is the adiabatic process?

The adiabatic process is a thermodynamic process in which there is no transfer of heat or matter between a system and its surroundings. This means that the system is isolated and does not exchange energy with its surroundings.

How does the adiabatic process work?

The adiabatic process works by changing the temperature and pressure of a system without any heat entering or leaving the system. This can be achieved by compressing or expanding a gas rapidly, which causes changes in temperature and pressure without any heat exchange.

What are some real-life examples of the adiabatic process?

The adiabatic process can be observed in various natural phenomena such as the formation of thunderstorms, the movement of air masses in the atmosphere, and the formation of clouds. It is also used in industrial processes such as gas turbines and refrigeration systems.

What are the differences between adiabatic and isothermal processes?

The main difference between adiabatic and isothermal processes is that adiabatic processes do not involve any heat transfer while isothermal processes occur at a constant temperature. Additionally, adiabatic processes tend to result in larger changes in temperature and pressure compared to isothermal processes.

How is the adiabatic process related to the first law of thermodynamics?

The first law of thermodynamics states that energy cannot be created or destroyed, only transferred or converted from one form to another. The adiabatic process follows this law as there is no transfer of energy (heat) in and out of the system, and any changes in temperature and pressure are a result of the conversion of energy within the system.

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