Respuesta :
Answer: The boiling point of solution is 101.56°C
Explanation:
Elevation in boiling point is defined as the difference in the boiling point of solution and boiling point of pure solution.
The equation used to calculate elevation in boiling point follows:
[tex]\Delta T_b=\text{Boiling point of solution}-\text{Boiling point of pure solution}[/tex]
To calculate the elevation in boiling point, we use the equation:
[tex]\Delta T_b=iK_bm[/tex]
Or,
[tex]\text{Boiling point of solution}-\text{Boiling point of pure solution}=i\times K_b\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}[/tex]
where,
Boiling point of pure water = 100°C
i = Vant hoff factor = 1 (For non-electrolytes)
[tex]K_b[/tex] = molal boiling point elevation constant = 0.52°C/m.g
[tex]m_{solute}[/tex] = Given mass of solute (urea) = 27.0 g
[tex]M_{solute}[/tex] = Molar mass of solute (urea) = 60 g/mol
[tex]W_{solvent}[/tex] = Mass of solvent (water) = 150.0 g
Putting values in above equation, we get:
[tex]\text{Boiling point of solution}-100=1\times 0.52^oC/m\times \frac{27\times 1000}{60\times 150}\\\\\text{Boiling point of solution}=101.56^oC[/tex]
Hence, the boiling point of solution is 101.56°C
A solution is prepared by dissolving 27.0 g of urea in 150.0 g of water has a boiling point of 101.54 °C.
The normal boiling point of water is 100 °C. However, when 27.0 g of urea is dissolved in 150.0 g of water, we expect the boiling point of the solution to be higher.
What is the boiling point elevation?
Boiling point elevation is the phenomenon that occurs when the boiling point of a liquid is increased when another compound is added. It is a colligative property. We can calculate the increase in the boiling point using the following expression.
ΔT = i × Kb × m
where,
- i is the Van't Hoff factor (i = 1 for nonelectrolytes).
- Kb is the molal boiling point constant (Kb = 0.513 °C/m for water).
- m is the molality.
What is molality?
Molality (m) is defined as the total moles of a solute contained in a kilogram of a solvent. We can calculate it using the following expression.
m = mass solute / molar mass solute × kg solvent
m = 27.0 g / (60.06 g/mol) × 0.1500 kg = 3.00 m
The boiling point elevation is:
ΔT = i × Kb × m = 1 × (0.513 °C/m) × 3.00 m = 1.54 °C
Then, the boiling point of the solution is:
T = 100 °C + 1.54 °C = 101.54 °C
A solution is prepared by dissolving 27.0 g of urea in 150.0 g of water has a boiling point of 101.54 °C.
Learn more about colligative properties here: https://brainly.com/question/10323760
