What is the vapor pressure (kPa) of water at 25 °C above an aqueous solution that is 10.6% by mass of glucose (molar mass = 180.2 g/mol)? The vapor pressure of pure water at 25 °C is 3.17 kPa. а. 3.168 b. 0.037 с. 3.133 d. 0.081 e. 3.064
What is the vapor pressure (kPa) of water at 25 °C above an aqueous solution that is 10.6% by mass of glucose (molar mass = 180.2 g/mol)? The vapor pressure of pure water at 25 °C is 3.17 kPa. а. 3.168 b. 0.037 с. 3.133 d. 0.081 e. 3.064
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question

Transcribed Image Text:**Understanding Vapor Pressure of an Aqueous Solution:**
**Problem Statement:**
What is the vapor pressure (kPa) of water at 25°C above an aqueous solution that is 10.6% by mass of glucose (molar mass = 180.2 g/mol)? The vapor pressure of pure water at 25°C is 3.17 kPa.
**Options:**
- **a.** 3.168
- **b.** 0.037
- **c.** 3.133
- **d.** 0.081
- **e.** 3.064
**Explanation:**
To solve this problem, one must use the concept of the colligative properties of solutions, specifically Raoult's Law, which relates the vapor pressure of a solution to the vapor pressure of the pure solvent and the mole fraction of the solvent in the solution.
**Steps to Calculate:**
1. Calculate the mass of glucose (solute) and water (solvent) in the solution:
- Assume we have 100 g of the solution.
- Mass of glucose = 10.6 g
- Mass of water = 100 g - 10.6 g = 89.4 g
2. Convert these masses to moles:
- Moles of glucose = \(\frac{10.6 \, \text{g}}{180.2 \, \text{g/mol}} = 0.0588 \, \text{moles}\)
- Moles of water = \(\frac{89.4 \, \text{g}}{18 \, \text{g/mol}} \approx 4.9667 \, \text{moles}\)
3. Calculate the mole fraction of water (solvent):
- Mole fraction of water \( (\chi_{water}) = \frac{\text{moles of water}}{\text{total moles}} \)
- Total moles = 0.0588 mol (glucose) + 4.9667 mol (water) = 5.0255 mol
- Mole fraction of water \( (\chi_{water}) = \frac{4.9667}{5.0255} \approx 0.9883 \)
4. Use Raoult's Law to find the vapor pressure of the solution:
- \(P_{solution
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 3 images

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning

Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY