Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Problem Statement:**
An aqueous solution contains **0.589 g** of dextran in **106 mL** of solution at **21°C**. It has an osmotic pressure of **1.47 mmHg**. What is the average molecular weight of the dextran?
**Calculation Required:**
You need to calculate the molecular weight of dextran in atomic mass units (amu).
**Input Box:**
- Molecular weight = [Input Field]
- Unit: amu
**Explanation:**
To find the molecular weight, you can use the formula for osmotic pressure:
\[
\Pi = \frac{nRT}{V}
\]
Where:
- \(\Pi\) is the osmotic pressure.
- \(n\) is the number of moles of solute.
- \(R\) is the ideal gas constant.
- \(T\) is the temperature in Kelvin.
- \(V\) is the volume of the solution in liters.
Convert the given information into the proper units, and use this relationship to solve for the molecular weight.](https://content.bartleby.com/qna-images/question/c57e455c-e356-45e8-9424-9ece1c8d9714/6319e38e-d1f4-4a92-976e-873f080e6cde/w8l1wqe_processed.png)
Transcribed Image Text:**Problem Statement:**
An aqueous solution contains **0.589 g** of dextran in **106 mL** of solution at **21°C**. It has an osmotic pressure of **1.47 mmHg**. What is the average molecular weight of the dextran?
**Calculation Required:**
You need to calculate the molecular weight of dextran in atomic mass units (amu).
**Input Box:**
- Molecular weight = [Input Field]
- Unit: amu
**Explanation:**
To find the molecular weight, you can use the formula for osmotic pressure:
\[
\Pi = \frac{nRT}{V}
\]
Where:
- \(\Pi\) is the osmotic pressure.
- \(n\) is the number of moles of solute.
- \(R\) is the ideal gas constant.
- \(T\) is the temperature in Kelvin.
- \(V\) is the volume of the solution in liters.
Convert the given information into the proper units, and use this relationship to solve for the molecular weight.
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