   # Urea, (NH 2 ) 2 CO, which is widely used in fertilizers and plastics, is quite soluble in water. If you dissolve 9.00 g of urea in 10.0 mL of water, what is the vapor pressure of the solution at 24 °C? Assume the density of water is 1.00 g/mL. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13, Problem 26PS
Textbook Problem
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## Urea, (NH2)2CO, which is widely used in fertilizers and plastics, is quite soluble in water. If you dissolve 9.00 g of urea in 10.0 mL of water, what is the vapor pressure of the solution at 24 °C? Assume the density of water is 1.00 g/mL.

Interpretation Introduction

Interpretation: The vapor pressure of solution has to be identified.

Concept introduction:

Raoult’s law: The vapor pressure of the solvent over the solution Psolvent is proportional to the mole fraction of the solvent. The ideal solution obeys the Raoult’s law.

PsolventχsolventPsolvent,where,Psolventisthevapor pressure of the solvent over the solution,χsolventis mole fraction of solvent in solution, Psolvent is the vapor pressure of the pure solvent.

### Explanation of Solution

Given data:

Mass of urea = 9 gVolume ofWater =10 mlPsolvent (vapor pressure of water at 24C ) =22.4 mmHg

Massofwater=(1.0 g/ml)(10 ml)=10g

Calculate the mole fraction of water in solution(χwater):nurea=9g60.06g/mol=0.150molnwater=10g18=0

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