Physics: Expansion at constant pressure

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SUMMARY

The discussion focuses on solving a physics problem involving the expansion of an ideal monoatomic gas at constant pressure. The initial volume is 2.30 m3, the final volume is 3.10 m3, the pressure is 1.71 atm, and the initial temperature is 300 K. The key equations used include the ideal gas law, PV=nRT, to find the number of moles (n) and the final temperature. Participants emphasize the importance of unit conversion and ensuring dimensional consistency throughout the calculations.

PREREQUISITES
  • Understanding of the ideal gas law (PV=nRT)
  • Knowledge of unit conversions (atm to N/m2, m3 to L)
  • Familiarity with concepts of thermodynamics related to gas expansion
  • Basic algebra for solving equations
NEXT STEPS
  • Practice unit conversion techniques in thermodynamic calculations
  • Explore the derivation and applications of the ideal gas law
  • Learn about reversible processes in thermodynamics
  • Study work done by gases during expansion and compression
USEFUL FOR

This discussion is beneficial for physics students, particularly those studying thermodynamics, as well as educators and anyone interested in understanding gas behavior under varying conditions.

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Homework Statement



An unknown number of moles of an ideal monoatomic gas expand reversibly from Vi = 2.30 m3 to Vf = 3.10 m3, at a constant pressure of 1.71 atm and an initial temperature of 300 K.
Find the number of moles of gas.
Find the final temperature of the gas K.
Calculate the work done by the gas.

Homework Equations



I'm using PV=nRT

The Attempt at a Solution



Converting the pressure in atm to N/m^2 and m^3 to L. I'm using the initial volume for V, 8.315 for R and the initial temp in K and solving for n. I keep getting the same answer and it is coming up wrong. Please help!
 
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Write out all the units during your calculation. Do the units make sense in the end? Also, this isn't advanced physics.
 

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