Ideal Gas Law: Total Pressure of Two Flasks

[@blakeamartin07]

Great video. Been looking for this explanation for an hour now. Now I need to look up temperature and boiling points. Lol

[@iit-jeephysics3782]

More easier way is to equate moles. Like final moles is equal to moles of hydrogen in 2nd + moles of nitrogen in 1st container. Temperature is constant for both. Use n=pv/RT in one go you will find total pressure

[@stephenniewong4635]

Nice, now i understand. Thank you!!

[@lunariameldovin3457]

What if it have a temperature

[@rutaremwa69]

what if they both had different initial temperature?

[@lalisaprettypretty]

Hello sir, how to calculate the number of moles of gas has flowed from one flask to the other?

[@chemistrysteps8270]

You could use the ideal gas law equation (PV = nRT) to calculate the initial moles based on the initial pressure in any of the flasks, and then use the equation again to calculate the moles in the same flask based on the final pressure. The difference should be what's flowed from one flask to the other. Just keep in mind that the flow is continuous in both directions.

[@julioherrera1258]

In real scenario the "empty" flask should have air in it, correct?

[@iit-jeephysics3782]

Even if there is air then again it will be distributed equal in both container so again total pressure will remain same in both containers. Value might differ but concept is same.

[@johnspence8141]

You should also note that SINCE total pressure = pressure (Nitrogen ) + pressure hydrogen, you can REWRITE total pressure = (P1*v1/V total + P2/V2/Votal ) = (P1*V1 +P2*V2)/V total . So TOTAL pressure = (1.8 *3 + 3.5 *2)/5 = 2.48 atm

[@rubybeau4774]

thanks

[@tuspaodds5755]

What if the volume doesn't change

[@whytfhhs8365]

how would that be possible?

[@abd9362]

Thanks broski

[@basilazeem974]

thx

[@shrabantichakrabartythakur9562]

Noicccc

[@kingyouki5524]

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