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- TL;DR Summary
- A monatomic and a diatomic gas, initially at the same temperature and pressure, are separated by a movable, heat-conducting wall in an adiabatic container. How do they reach equilibrium?
Consider an adiabatic container divided into two chambers by a movable, heat-conducting wall. One side contains a monatomic ideal gas, while the other contains a diatomic ideal gas. Initially, both gases are at the same temperature and pressure. Over time, the wall moves until a new thermodynamic equilibrium is reached.
- How can the final position of the wall be determined based on the thermodynamic properties of the gases?
- Will the final temperatures of the two gases be the same? If not, what physical principle justifies this difference?
- If the gases were real instead of ideal, how might the system’s behavior deviate from the predictions of the ideal gas model?