15.) Which of the following systems has the greatest change in internal energy? A.) A mixing of two ideal diatomic gases with equimolar amount and the same temperature and pressure. B.) An isolated container that contains two gases of different pressures separated by a frictionless and movable piston. The gases are allowed to reach a mechanical equilibrium. C.) Two blocks of similar metal that are in contact in an isolated container, one block metal has a temperature of 100°C while the other block of metal has a temperature of 20°C. The two blocks of metals are allowed to reach thermal equilibrium. D.) An ideal gas that was allowed to expand freely and adiabatically. E.) None of these.

15.) Which of the following systems has the greatest change in internal energy? A.) A mixing of two ideal diatomic gases with equimolar amount and the same temperature and pressure. B.) An isolated container that contains two gases of different pressures separated by a frictionless and movable piston. The gases are allowed to reach a mechanical equilibrium. C.) Two blocks of similar metal that are in contact in an isolated container, one block metal has a temperature of 100°C while the other block of metal has a temperature of 20°C. The two blocks of metals are allowed to reach thermal equilibrium. D.) An ideal gas that was allowed to expand freely and adiabatically. E.) None of these.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.66E: In orbit about Earth, a weather balloonjettisons a weight andascends to a higher altitude. If the...

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In orbit about Earth, a weather balloonjettisons a weight andascends to a higher altitude. If the initial pressure inside the balloon is 0.0033 atm and it ascends to an altitude where the pressure is 0.00074 atm, by what fraction does the absolutetemperature change? Assumethat the balloon is filled with helium, a good approximation of an ideal gas, and that the change is adiabatic.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
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