[ctpengage]

Two 5dm^3 flasks are connected by a narrow tube of negligible volume. Initally the two flasks are both at 300K and contain a total of 2 moles of an ideal gas. One flask is heated to a uniform temperatiure of the 400K while the other is kept at 300K. Assuming their volume does not alter , calculate the no. of moles of gas in each flask of the gas and the final pressure.

I was stuck on this for ages until I finally decided to try it by assuming the pressures were equal. However why is the pressure equal in each flask of gas.

[Borek]

Assuming pressures are not identical - what will happen?

[Controlled Substance]

Good assumption.

Keep in mind that pressure is caused by the collision of gas particles against its container.

What would happen if you'd have a low pressure (empty) balloon fixed to one side of a straw, and then you fix a full balloon to the other side? (Both balloons are fixed in a way where air can travel through the straw.) What will each balloon look like afterwards?

[ctpengage]

Pressure equalises out don't it?

[Borek]

Pressure equalises out don't it?

Now read your own question from the very first post.