
Interpretation:
The grams of urea required to prepare solution in
Concept introduction:
Raoult’s law: Raoult’s law states that solvent partial pressure over a solution is equal to vapor pressure of pure solvent multiplied with mole fraction of the solvent.
Where,
Moles: One mole is equivalent to the mass of the substance consists same number of units equal to the atoms present in
From given mass of substance moles could be calculated by using the following formula,
Mass: It is the quantitative measure of a substance. The amount of matter present in substance is expressed as mass. The
Density is calculated by mass of the substance divided by its volume.

Answer to Problem 12.54QP
The grams of urea required to prepare solution is
Explanation of Solution
Given data: Mass of
Vapor pressure
Temperature
Vapor pressure of
Calculate mole fraction of urea:
Substitute the solvent vapor pressure value and vapor pressure value of pure solvent into Raoutl’s Law equation to calculate mole fraction.
Calculate moles of water:
Calculate moles of urea:
Substitute the mole fraction of urea and the water moles into mole fraction equation to calculate the moles of urea.
Convert moles of urea into mass:
Therefore, the mass of urea is
The grams of urea required to prepare solution in
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Chapter 12 Solutions
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