What is the boiling point of a solution composed of 19.0 g of urea, (NH₂)2 CO, in 0.500 kg of water? (Kbp for H₂O is +0.5121 °C/m.) Boiling point = °C
What is the boiling point of a solution composed of 19.0 g of urea, (NH₂)2 CO, in 0.500 kg of water? (Kbp for H₂O is +0.5121 °C/m.) Boiling point = °C
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Problem Statement:**
What is the boiling point of a solution composed of 19.0 g of urea, (NH₂)₂CO, in 0.500 kg of water? (K<sub>bp</sub> for H₂O is +0.5121 °C/m.)
**Solution:**
Boiling point = ☐ °C
---
**Analysis:**
To determine the boiling point of the solution, you need to calculate the molality of the urea in the water and then use the boiling point elevation formula:
1. **Calculate molality (m):**
\[
\text{molality (m)} = \frac{\text{moles of solute}}{\text{kilograms of solvent}}
\]
2. **Determine the moles of urea:**
- Molar mass of urea, (NH₂)₂CO = 60.06 g/mol
- Moles of urea = \(\frac{19.0 \text{ g}}{60.06 \text{ g/mol}}\)
3. **Use the boiling point elevation formula:**
\[
\Delta T_b = i \cdot K_{bp} \cdot \text{molality}
\]
- For non-electrolytes like urea, \(i = 1\).
4. **Calculate the new boiling point:**
- New boiling point = 100°C + ΔT<sub>b</sub> (since the normal boiling point of water is 100°C).
Complete these calculations to find the final boiling point.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5e64e050-9cb6-467e-8132-ec94d7497579%2Ff3d37b89-e72f-44c8-91dd-8d6b544c0fd8%2Fyugq7fl_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
What is the boiling point of a solution composed of 19.0 g of urea, (NH₂)₂CO, in 0.500 kg of water? (K<sub>bp</sub> for H₂O is +0.5121 °C/m.)
**Solution:**
Boiling point = ☐ °C
---
**Analysis:**
To determine the boiling point of the solution, you need to calculate the molality of the urea in the water and then use the boiling point elevation formula:
1. **Calculate molality (m):**
\[
\text{molality (m)} = \frac{\text{moles of solute}}{\text{kilograms of solvent}}
\]
2. **Determine the moles of urea:**
- Molar mass of urea, (NH₂)₂CO = 60.06 g/mol
- Moles of urea = \(\frac{19.0 \text{ g}}{60.06 \text{ g/mol}}\)
3. **Use the boiling point elevation formula:**
\[
\Delta T_b = i \cdot K_{bp} \cdot \text{molality}
\]
- For non-electrolytes like urea, \(i = 1\).
4. **Calculate the new boiling point:**
- New boiling point = 100°C + ΔT<sub>b</sub> (since the normal boiling point of water is 100°C).
Complete these calculations to find the final boiling point.
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