Calculate the freezing-point depression and osmotic pressure at 258C of an aqueous solution containing 1.0 g/L of a protein (molar mass 5 9.0 3 104 g/mol) if the density of the solution is 1.0 g/cm3. b. Considering your answer to part a, which colligative property, freezing-point depression or osmotic pres- sure, would be better used to determine the molar masses of large molecules

0.2 atm is the osmotic pressure.  Decreased freezing point since an exact number of moles could be determined, osmotic pressure would be a better method for determining the molar masses of a big molecule.

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The osmotic pressure is 0.2 atm

The freezing point depression=2*10^-5 \

Osmotic pressure would be better to determine the molar masses of large molecule as precise number of moles can be known.

Explanation:

The equation for the osmotic pressure is the:

π=MRT

 where π= osmotic pressure

           M= Molarity , R= Gas constant, T =temperature

M= 1/9*10^4

   = 1.1*10^-5 mol/litre

    π= MRT

      = 1.1*10^-5*0.0826* 298*760 Torr

       =  0.20 torr

      osmotic pressure= 0.20 atm

ΔTf=Kfm*

 = 1.86*1.1.10^-5

=2.06*10^-5

The osmotic pressure would be better to determine the molar mass from the formula π= MRT

When molarity is known molar mass ie easily known as number of moles would be known and multiplied with atomic weight will give molar mass.

the atomic mass is the bottom number on the element.

-steel jelly

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

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