Two samples of a monatomic ideal gas are in separate containers at the same conditions of pressure, volume, and temperature (V = 1.00 L and P = 1.00 atm). Both samples undergo changes in conditions and finish with V = 2.00 L and P = 2.00 atm. However, in the first sample, the volume is changed to 2.0 L while the pressure is kept constant, and then the pressure is increased to 2.00 atm while the volume remains constant. In the second sample, the opposite is done. The pressure is increased first, with constant volume, and then the volume is increased under constant pressure.
-Calculate the difference in $\Delta$E between the first sample and the second sample.

Question

Quizplus · Accepted Answer

The work done on or by the gas is path-dependent. However, the change in internal energy for an ideal gas depends only on the initial and final states, not on the path taken. Since both samples start and end at the same conditions, the change in internal energy is the same for both, resulting in a difference of zero.

Two Samples of a Monatomic Ideal Gas Are in Separate Δ\DeltaΔ

Two Samples of a Monatomic Ideal Gas Are in Separate $\Delta$