What External Pressure Is This Gas Expanding Against?

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SUMMARY

The discussion centers on a thermodynamics problem involving a piston containing 21.9 g of nitrogen gas (N2) with a molecular weight of 28.02 g/mol. The initial volume is 7.27 L, and after adding 849.5 J of heat, the temperature rises by 37.3 °C, resulting in a volume change of 0.839 L. The change in internal energy (ΔE) for this process is 607.2 J. The external pressure against which the gas expands can be calculated using the formula for work done during expansion, and the heat added is consumed by both increasing the internal energy and doing work on the piston.

PREREQUISITES
  • Understanding of the ideal gas law
  • Familiarity with the first law of thermodynamics
  • Knowledge of specific heat capacity calculations
  • Basic principles of work done by gases during expansion
NEXT STEPS
  • Calculate the external pressure using the formula: P = ΔE / ΔV
  • Learn about the first law of thermodynamics and its application in closed systems
  • Study specific heat capacity and its role in thermodynamic processes
  • Explore the concepts of work and heat transfer in gas expansion scenarios
USEFUL FOR

This discussion is beneficial for students and professionals in chemistry and physics, particularly those studying thermodynamics, as well as engineers working with gas systems and energy transfer processes.

heylookitsnes
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Can someone help me with this problem? Even if you could just tell me the steps I'd need to take.. or even just an equation. Something please?

A piston filled with 21.9 of N2 g (MW = 28.02 g/mol) has an initial volume of 7.27 L. 849.5 J of heat were added to the piston, which increased the temperature of the gas by 37.3 °C, leading to a volume change of 0.839 L. The value of ΔE for this expansion process was 607.2 J. What external pressure is this gas expanding against? (The specific heat of N2 g is 1.04 J/g °C)
 
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Added heat was consumed by two processes. Can you name them? Calculate how much energy each of the processes used?
 
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