Question

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A solution containing 6g of a solute in 300cm^3 of water gave an osmotic pressure of 5.5atm at 27°C .Calculate the boiling point of the solution. The molal elevation constant for water is 0.52°C per 1000g​

Answer 1

Answer:

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Explanation:

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Answer 2

Answer:

Osmotic presuure= i∗C∗R∗T

where, C=concentration of solute(in terms of Molarity)

R= Gas constant =0.082L(atm)(mol)^−1K^−1

T=temperature (in Kelvin)

i=Van’t-Hoff factor(=1 for non-electrolyte)

5% urea solution means 5g urea is present in 100ml of solution.

Mole of urea=weight/Molecular weight of urea

=5g/60gmol^−1=112

Hence Concentration of urea

(in terms of Molarity)

= (moles of urea(n) /volume of solution ) ×1000

={(112)/100}∗1000

=1012

Hence Osmotic pressure =1×(10/20)×0.082×300 atm

=20.52atm