A solution of a non-volatile solute in water has a boiling point of 375.3K. Calculate the vapour pressure of water above this solution at 338K. Given, p_(0) (water) = 0.2467 atm at 338K and K_(b) for water = 0.52.

A solution of a non-volatile solute in water has a boiling point of 37

1.	A solution of a non-volatile solute in water has a boiling point of 375.3K. Calculate the vapour pressure of water above this solution at 338K. Given, p_(0) (water) = 0.2467 atm at 338K and K_(b) for water = 0.52.
Answer» <html><body><p></p>Solution :`DeltaT_(b)=(375.3-373.16)=2.15K` <br/> We know that, <br/> `DeltaT_(b)`= Molality `<a href="https://interviewquestions.tuteehub.com/tag/xx-747671" style="font-weight:bold;" target="_blank" title="Click to know more about XX">XX</a> K_(b)` <br/> 2.15 = Molality `xx 0.52` <br/> Molality `= (2.15)/(0.52) = 4.135` <br/> i.e., 4.135 moles of the <a href="https://interviewquestions.tuteehub.com/tag/solute-1217068" style="font-weight:bold;" target="_blank" title="Click to know more about SOLUTE">SOLUTE</a> present in 1000g of water (55.5 moles) <br/> Mole fraction of water `= (55.5)/(4.135+55.5)=(55.5)/(59.635)` <br/> <a href="https://interviewquestions.tuteehub.com/tag/vapour-1442886" style="font-weight:bold;" target="_blank" title="Click to know more about VAPOUR">VAPOUR</a> pressure of water above solution <br/> = Mole fraction `xx p_(0)` <br/> `=(55.5)/(59.635)xx0.2467=0.23`atm.</body></html>