pls explain the formula involved wo rigid boxes containing different ideal gases are placed on a table. Box A contains one mole of nitrogen at temperature, while Box B contains one mole of helium at temperature (7/3) T0. The boxes are then put into thermal contact with each other and heat flows between them until the gases reach a common final temperature. (Ignore the heat capacity of boxes). Then, the final temperature of the gases,, in terms ofis Share with your friends Share 6 Jyoti Pant answered this The change in internal energy of an ideal gas is given by,∆U=nCv∆T=nCv (Tf-Ti)Where,n=Number of molesTf=Final temperatureTi=Initial temperatureFor nitrogen (diatomic gas),Cv=52RFor helium(monoatomic gas)Cv=32RSince no heat is given or taken from the surrounding, the total internal energy of the system can't change.Thus,∆U(For nitrogen)+∆U(For helium)=0or 1×52R×(Tf-T0)+ 1×32R×(Tf-7T03)=0or Tf=32T0 18 View Full Answer Ratna Manjula answered this The question is Two rigid boxes containing different ideal gases are placed on a table. Box A contains one mole of nitrogen at temperature T0, while box B contains one mole of helium at temperature (7/3) T0. The boxes are then put into thermal contact with each other, and heat flows between them until the gases reach a common final temperature (Ignore the heat capacity of boxes). Then, the final temperature of the gases, Tf, in terms of T0 -7
