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Lena772
 one year ago
Determine the osmotic pressure (in atm) , at 80.2 o F, of an aqueous Iron (II) nitrate solution whose mole fraction of solute is 0.002696.
Density solution = 1.11 g/mL
Lena772
 one year ago
Determine the osmotic pressure (in atm) , at 80.2 o F, of an aqueous Iron (II) nitrate solution whose mole fraction of solute is 0.002696. Density solution = 1.11 g/mL

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Lena772
 one year ago
Best ResponseYou've already chosen the best response.1PV= nRT So Posm = nRT/V R= 0.08206 L*atm/mol*k T= 80.2F = 299.928 K V = calculate somehow using density n = reverse mole fraction calculation to find total moles of solution

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1@taramgrant0543664 @photon336 Can you guys assist me in reversing the mole fraction equation to find total moles of solution and then using that calculation with the density to find volume?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0V=m/d where v is volume, m is mass and d is density

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1right, but i can't find the mass of the solution until i reverse the mole fraction and find moles of total solution

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1I think? Mole fraction = (moles solute) / (moles solute + moles solv ). We are given moles of solute, but I don't know where to go from here. :(

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Yes that is the formula

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0You're not given moles of solvent?

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1@Abhisar @pooja195 @zepdrix @abb0t

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Hmmm... I don't know to tell you sorry I've only touched on osmotic pressure stuff none of my profs or teachers really talked much about it so I don't want to lead you on the wrong direction

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1Do you know anyone online that can help me? @taramgrant0543664

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0I think you got a majority of the ones that could hopefully help

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1@abb0t Do you think you can help me?

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1@NoelGreco Hi! Can you please help me?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4@Lena772 can you find out molality ?

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1yes moles solute/kg solvent. But I don't know the moles of solute.

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4Here is a formula : \[\large \bf Molality=\frac{X_{solute}\times 1000 }{(1X_{solute}) \times M_{solvent}}\]

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4and then use this : \[\large \bf Molarity=\frac{molality \times density \times 1000}{molality \times Molar~ mass~ of~ solute+1000}\]

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4hope you can find molarity

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1Molal = (0.002696 mol Solute * 1000) / ( 0.997304 * molality of solvent) , BUT idk the molality of the solvent

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4its molar mass of solvent

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4not molality of the solvent Remember molality is denoted by small m i.e `m`

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1Molal = (0.002696 mol Solute * 1000) / ( 0.997304 * 175.8948)

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4after you find out molarity ! Use this : \[\large \bf Osmotic~Pressure(\pi)=Molarity \times RT \times vant~hoff~factor\]

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4i don't know. Use calculator

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4i am here to give you HINTS as possible

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1molality = 0.94396197 0.94396197 * 0.08206 * 299.928 K * van hoult?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4you don't know vant hoff factor ?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4@Lena772 then first learn this term and then solve the rest of question

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1Would the factor be 4 because there is 3 pieces of iron nitrate and 1 piece of water molecule?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4nope ! try again

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1What's wrong about it?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4see the oxidation state of iron in question. You took the oxidation state as +3

Lena772
 one year ago
Best ResponseYou've already chosen the best response.1I get 69.7 atm. That's sounds extreme. Can you just plug those in and see if you get the same value?

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4lol but i don't have much time to solve ! Sorry ! Better luck ,Next time

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4i have to go now ! Bye ! @Lena772 Its been a nice time with you ! :)

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4MEDAL for your HARDWORK and keen interest on solving this question !

mayankdevnani
 one year ago
Best ResponseYou've already chosen the best response.4REMEMBER : Don't suppose that i am a professor, i am (18)
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