The change of internal energy of air in a car rubber can be calculated using the formula U = (5/2)nRT, where n is the number of moles of air. Given a volume of 50 liters, an initial pressure of 1.8 atm, and a temperature of 293 K, the number of moles (n) is determined to be approximately 3.7. After the pressure increases to 2 atm, the change in internal energy is calculated to be 2500 J, which aligns closely with the textbook answer of 2537 J when accounting for significant figures and using precise values for atmospheric pressure.
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Ok but how can I find the U with this compound of gases like air?TSny said:Don't forget the ideal gas law. Also, in the formula for U, are you sure the fraction is 3/2? Nitrogen and oxygen are diatomic gases.
I am writing my solution: pV=nRT=>n=(1.8*10^5*0.05)/(8.31*293)=3.7TSny said:Don't forget the ideal gas law. Also, in the formula for U, are you sure the fraction is 3/2? Nitrogen and oxygen are diatomic gases.