Vapor pressure example | Chemistry | Khan Academy
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- เผยแพร่เมื่อ 27 ธ.ค. 2024
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Vapor pressure example using the ideal gas law. Created by Sal Khan.
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Chemistry on Khan Academy: Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity. This material roughly covers a first-year high school or college course, and a good understanding of algebra is helpful.
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I watched this same video in highschool, undergrad and now in post grad.
I hate chemistry but love khan
And looks like you never learned 😂
watching in highschool, vapor pressure is the one thing that confused me in Chemistry 1
@dalcde yes
By the other volume I assume you mean the 2 L of water that you put in the room? The reason you use the volume of the room instead is that the room is the volume that will hold the water vapor, and since the water vapor will exert some pressure on the water in the container, you need to figure out its pressure. Since the vapor is in the room, you use the room's volume.
From what I understand, the only thing that affects evaporation at a given temperature is the pressure of water vapor on the surface of the water. If the atmospheric pressure drops below the vapor pressure, the water will start boiling instead of simply evaporating.
I've learned a lot from many of your video's keep up the good work!
that was awesome thank you
thanks for the example! helped me quite a lot actually!
i can't believe my professor didn't bother to go through any of this... it's not actually that hard once someone explains it to you in a rational way
this was super helpful to me
I don't think you're using "alas" quite right there, but I'm glad to hear that all the same!
what calculator apps are you using??
Love you! Thanks for this help.
Nice 😊
In the assumptions, shouldn't we say the room is a vacuum ie no air in it?
you did it as a "mysterious formula?" lol youre the best
very good
Sir, why u took room volume as vapour volume? There is still some water also consuming the room volume.
Tankxx lot
you're right
i love you sal!
I'm in college chem 1 and on our practice exam answer sheet he has the water vapor pressure, but it is not given in the problem. NO where in the book or lecture does it say how to obtain the pressure per degree's C. Anyone have answer for this, or do you think my professor is giving us a table?
How much time does it take to evaporate ?
thanks
maybe i"m a little out of it, ut why did you use that volume again versus the other volume?
Your explanation didn't take the effect of atmospheric pressure. What if we change the room's inside pressure. Please explain.
But isn't it always the case that at a particular vapor pressure (as long as atmospheric pressure is higher) by definition the same number of liquid molecules go into gas and gas goes into liquid? So it will never completely evaporate?
Good question, but you actually can get complete evaporation. This happens when the glass of water is sitting outside, the water will begin to evaporate but the water vapor will diffuse into the atmosphere and never build a large enough partial pressure to reach the vapor pressure (I.e. equilibrium)
so what if they ask you for milligrams and give u volume (1.00-L flask)
and then give you 2.00 mg of I2 and ask for the final pressure.....??
A 0.964 gram sample of a mixture of sodium formate and sodium chloride is analyzed by adding sulfuric acid. The equation for the reaction for sodium formate with sulfuric acid is shown above. The carbon monoxide formed measures 242 milliliters when collected over water at 752 torr and 22.0°C (vapor pressure of water at 22.0°C = 19.8 torr). Calculate the percentage of sodium formate in the original mixture. i need help
are we assuming here that the inicial pressure of the room was 0?, i mean if we were talking about a realistic case the pressure in the dormitory room would be about 1 atm, well thats way above 0.0313 atm ... im confused xD Help!! pls!!
Didn't get that as well.. maybe sum 0.0313 atm with the current pressure, giving 1,0313 atm as we can sum the pressure of different gases to give the total pressure. So initially the pressure was 1 atm, and after all the water had evaporated the pressure was 1,0313 atm.
im confused why and how did we get 0.0313 atm?
1 atm = 760 mm Hg
1 mm Hg = 1/760 atm
23.8 mm Hg = 23.8*(1/760) atm = 0.0313 atm
This channel belongs to which country?