Daltons Law of Partial Pressures and Henry’s Law Solubility Chemistry MCAT

[@tanvirlatif3203]

You are a GOD. You deserve exponentially more subscribers!

[@screamingperson8188]

Thank you so so much 💗! You explained it so well that I feel that I must have been an idiot before for not understanding it 🙈

[@kevuseth8027]

All Hail Science Simplied, the patron Saint of the C/P MCAT Section!

[@gooddeedsleadto7499]

Stripper colums in petrochemical refineries use Dalton’s law of partial pressure principle in the distillation process by adding steam into the mix in the column.

[@imosdefinite]

Can I ask how you developed this high level of mastery over this material so much so that you're able to explain it so easily?! aka - how do you go about learning new stuff? I'd love to see a video on how you're navigating med school and the ways you study new material.

[@sciencesimplified3890]

I’ve been meaning to post a video about study habits I’ve developed through medical school, I will at some point! Honestly at the end of the day nothing can replace putting in time and effort and forcing yourself to have consistent study habits, I swear studying 3 hours a day (however with no exceptions) is plenty to get into med school in my opinion the key is consistency and not procrastinating!

[@imosdefinite]

@@sciencesimplified3890 yess! Excited for that video to drop! teaaach us

[@FrontierThesisYU]

6:45 is the beginning of the discussion of Henry's Law

[@poojachaudhari1331]

This video deserves more likes

[@banwaita6723]

Would a question ever ask for the mole fraction of a single atom of Oxygen? Or would that not be possible because it's diatomic? If the former is true, then how would you solve for that? By further halving the mole fraction?

[@sciencesimplified3890]

Yes the way you described it is the way you would solve it. I believe if you have a question like this on the MCAT they would make it clear what they’re specifically looking for and as long as you understand the concept I think you’ll be good!

[@jiinjung1445]

Doesn't partial pressure of a gas change with absence or presence of other gases though? - as we have to consider the total number of mole in the solvent when we calculate the partial pressure of each gas. - I thought molarity of a gas in a solution would therefore increase with the absence of the other gas?

[@sciencesimplified3890]

im a little confuse what youre asking.. but all gasses act independent of other gasses, they act as if every other gases in the system doesnt exist (this is an approximation and more exact accurate measurements its a bit more complex) but for all intents and purposes partial pressure of oxygen has no effect on nitrogen or co2 or other gases

[@jiinjung1445]

10:42 If we make N2 gas disappear from the system, wouldn't Molarity of So2 gas increase instead of staying the same? - as partial pressure of So2 would imcrease as a result. Thank you for your answer by the way.

[@sciencesimplified3890]

@@jiinjung1445 no, if you made N2 gas disappear, it would have no effect on the partial pressure of SO2 gas.. and therefore it would have no effect on SO2 molarity... Every gas has 0 effect on other gasses.. each gas does its own thing 100% independent from other gasses

[@jiinjung1445]

@@sciencesimplified3890 Thank you very much for your explanation. I thought if I make N2 gas disappear, the partial pressure of SO2 gas might increase, as the number of total mole would decrease, making the denominator smaller...

[@sciencesimplified3890]

If N2 disappeared, the mol fraction of SO2 would go to 100%... but if N2 disappeared the total pressure would decrease also... so S02 would contribute 100% to a new smaller total pressure

[@Tert-Butyl]

You sound like a slightly nerdier American STEM oriented Jordan Peterson. (intended as a compliment)