Calculating Internal Energy & Temperature Change of Ideal Gas

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SUMMARY

The discussion centers on calculating the change in internal energy and temperature change of an ideal gas using the first law of thermodynamics. The work done on the gas is 4.675x10^5 J, with heat transferred into the system at 2.95x10^6 J and heat lost to the environment at 7.95x10^6 J. The relevant equations include U = 3/2 nRT and ΔU = Q - W, where R is the ideal gas constant (8.314 J/mol·K). The participants explored different approaches to calculate the net heat transfer and the final temperature of the gas.

PREREQUISITES
  • Understanding of the first law of thermodynamics
  • Familiarity with ideal gas laws
  • Knowledge of heat transfer concepts
  • Basic algebra for solving equations
NEXT STEPS
  • Study the first law of thermodynamics in detail
  • Learn how to apply the ideal gas law in various scenarios
  • Explore the concept of internal energy in thermodynamic systems
  • Practice solving problems involving heat transfer and work done on gases
USEFUL FOR

This discussion is beneficial for students studying thermodynamics, physics enthusiasts, and anyone involved in engineering or physical sciences who needs to understand the behavior of ideal gases under varying conditions.

Nick88

Homework Statement


What is the change in internal energy (in Joules) of an ideal gas that does 4.675x10^5J of work, while 2.95x10^6J of heat is transferred into the system and 7.95x10^6J of heat is transferred from the system to the environment? Calculate the change in temperature of the two moles of the gas. (R=8.314 J/mol.k)

Homework Equations


Formulas on equation sheet relating to concept: U=3/2 nRT, change in U=Q-W

The Attempt at a Solution


Me and my friend attempted two different ways, I'm probably wrong but my setup was
4.675x10^5=8.314(1)(T)
2.95x10^6=8.314(1)(T)
I found the two answers and added then together and did 7.95x10^6=8.314(2)(T) found this answer, then subtracted the two answers to get a final temperature.
 
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What is the net amount of heat transferred to the gas? From the first law, what is the change in internal energy?
 

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