Isobaric Expansion: Finding Internal Energy & Heat w/ 2.0 Moles Ideal Gas

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SUMMARY

The discussion focuses on calculating the change in internal energy and heat during an isobaric expansion of a monatomic ideal gas with 2.0 moles. The work done by the gas is -3600 J, and the change in temperature is determined to be 216.6 K using the ideal gas law (PV=nRT). To find the change in internal energy (ΔU) and heat (Q), the First Law of Thermodynamics is applied, utilizing the relationship ΔU = Q - W, where W is the work done by the gas.

PREREQUISITES
  • Understanding of the First Law of Thermodynamics
  • Familiarity with the ideal gas law (PV=nRT)
  • Knowledge of isobaric processes in thermodynamics
  • Concept of monatomic ideal gases and their properties
NEXT STEPS
  • Study the First Law of Thermodynamics in detail
  • Learn how to calculate heat transfer in isobaric processes
  • Explore the properties of monatomic ideal gases
  • Investigate the relationship between work, heat, and internal energy
USEFUL FOR

This discussion is beneficial for students and professionals in thermodynamics, particularly those studying gas laws, heat transfer, and energy calculations in ideal gas systems.

jesuslovesu
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I have a Pressure vs Volume Graph and A -> B.
It's just an isobaric expansion, the work done by the gas is -3600 J.
The gas is monatomic ideal (2.0moles).
If I used it correctly, PV=nRT, I found the change in temperature to be 216.6K.

My question is: How do I find the change in internal energy and heat? I don't have any info about the gas except that it's ideal and 2.0 moles worth.
 
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Use the equation for the amount of heat required to change the temperature of that gas (at constant pressure). You will have W and Q, then find delta U using the First Law.
 

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