The problem involves a sealed 1L container of air initially at 20°C and 1 atm, which is placed in boiling water to reach thermal equilibrium before being opened. The question seeks to determine how many moles of air escape upon opening the container.
Several participants have offered guidance on using the ideal gas law and have raised questions about the physical behavior of air in the context of temperature differences. There is an exploration of potential scenarios regarding how air might escape or be replaced when the container is opened.
Participants note ambiguities in the problem setup, such as the effects of gravitational fields on air movement and the implications of opening the container in different ways (e.g., a small hole versus fully opening it). There is also mention of course materials that may provide additional context for the problem.
Yes. I guess that's right. But the rapid outrush would happen first, and then the natural convection would happen slowly. However, strictly speaking, the equilibrium would be unstable in a gravitational field.Simon Bridge said:@Chestermillar: that's probably what is intended all right - however, what is stopping all the hot air in the container leaving and cold air flowing in? Try it and see what happens? Maybe the container is opened at the bottom?
Simon Bridge said:@Chestermillar: strictly speaking, the equilibrium (internal-external pressure) would be unstable anyway - but, in a gravitational field you get the hot-air wanting to float. And, with that, we've basically done the question for OP :)