The discussion revolves around calculating the change of internal energy of air within a car tire, initially at a pressure of 1.8 atm and a temperature of 293 K, which later increases to 2 atm due to friction during travel.
Some participants have provided guidance on using the ideal gas law and have pointed out potential issues with significant figures in the calculations. There is acknowledgment of differing results from the textbook, leading to further exploration of the calculations involved.
Participants note that some data in the problem is given to only two significant figures, which may affect the final answer. There is also discussion about the appropriate value to use for atmospheric pressure in calculations.
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.