What are the final pressure for the gas?

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Homework Help Overview

The discussion revolves around an ideal diatomic gas undergoing adiabatic expansion. The original poster presents a scenario where a 1.00-mol sample of gas expands to twice its initial volume, seeking to determine the final pressure and temperature of the gas.

Discussion Character

  • Exploratory, Assumption checking, Problem interpretation

Approaches and Questions Raised

  • The original poster expresses uncertainty about applying the provided equation for adiabatic expansion. Some participants suggest using the ideal gas equation to find relationships between pressure, volume, and temperature.

Discussion Status

Participants are actively discussing various approaches to find the final temperature after determining the final pressure. There is a mix of suggestions regarding the use of different equations, but no consensus has been reached on a specific method to proceed.

Contextual Notes

There is a noted lack of numerical values for the initial volume, which some participants highlight as a constraint in solving the problem. The original poster's request for guidance indicates a need for clarification on the application of the equations involved.

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Homework Statement


A 1.00-mol sample of an ideal diatomic gas, originally at 1.00 atm and 15 celsius, expands adiabatically to 2.00 times its initial volume.

What are the final pressure for the gas? (Assume no molecular vibration.)
What are the final temperature for the gas?


Homework Equations



lnP + gamma lnV = constant

The Attempt at a Solution



I don't know how to use this equation and its the only one given in the adiabatic expansion section of my book. Can someone please guide me through. Thanks!
 
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I was able to solve for the final pressure. can you please show me how to find the final temperature. Thanks!
 


Just use the ideal gas equation again. You've know V_2 = 2V_1
 
Last edited:


but the no numerical value for volume is given...
 


Use the ideal gas equation to find V_1
 


You could also use the equation involving P, T and gamma. Using the ideal gas equation afterwards is a good check though.
 

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