The discussion revolves around the relationship between internal energy and pressure in a sealed container, specifically in the context of an ideal gas scenario. The original poster presents a problem involving initial conditions of volume, temperature, and pressure, and queries how doubling the internal energy affects the final pressure.
Participants are actively engaging with the problem, raising questions about the assumptions made regarding ideal gas behavior and the relationships between pressure, volume, and temperature. There is no explicit consensus yet, as different interpretations are being considered.
Participants are considering the implications of the ideal gas law and the conditions under which internal energy changes affect pressure, highlighting the need for clarity on whether the gas behaves ideally and the constraints of the problem setup.
If you change the volume, and hence the pressure, isothermally then the internal energy will not change. But if the volume stays the same then pressure and temperature can only vary if the other does too. Here, internal energy is being increased, so the temperature is going up, but the volume stays the same. So what happens to the pressure?ab94 said:I thought pressure was independent of Internal Energy so it would remain unchanged? but Idk
It depends. Is this an ideal gas? Can you explain your answer in terms of the ideal gas law?ab94 said:The pressure would also double?