How do you do this chemistry problem?

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New member
shouldn't we have the tempereture it boils at atmosphere's pressure.
I don't know maybe you should estimate it with water's boiling point.
 
Heres the problem:

An aqueous solution that is 0.205 m urea [CO(NH2)] is found to boil at 100.025 degrees C. Is the prevailing barometric pressure above or below 760.0 mmHg?

[Hint: At what temperature should the solution begin to boil if atmospheric pressure is 760.0 mmHg]

Answer: lower than 760 mmHg

Could someone explain how to do the problem and get the answer? Thanks.
 
delta T = kb x m = 0.512 x 0.205 =0.105 °C
boiling point at 1 atm (760 mm Hg) = 100 + 0.105 = 100.105 °C

because the boiling point of the solution is less than 100.105 the pressure would be lower
 
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