If 2.98 g of a non-electrolyte produces an osmotic pressure of 599 mm Hg when dissolved in enough water to produce 183 ml of solution at 35.6 °C, what is the molar mass of the non-electrolyte? Report the answer to 3 sig figs and in g/mol. A Moving to another question will save this response. « < Question 10 of 34
If 2.98 g of a non-electrolyte produces an osmotic pressure of 599 mm Hg when dissolved in enough water to produce 183 ml of solution at 35.6 °C, what is the molar mass of the non-electrolyte? Report the answer to 3 sig figs and in g/mol. A Moving to another question will save this response. « < Question 10 of 34
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![### Determining Molar Mass Based on Osmotic Pressure
**Question Prompt:**
If 2.98 g of a non-electrolyte produces an osmotic pressure of 599 mm Hg when dissolved in enough water to produce 183 mL of solution at 35.6 °C, what is the molar mass of the non-electrolyte? Report the answer to 3 significant figures and in g/mol.
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Question 10 of 34
---
**Explanation for Calculation:**
To determine the molar mass of the non-electrolyte, you need to use the formula for osmotic pressure:
\[
\pi = i \cdot M \cdot R \cdot T
\]
Where:
- \( \pi \) is the osmotic pressure.
- \( i \) is the van't Hoff factor (which is 1 for non-electrolytes).
- \( M \) is the molarity of the solution.
- \( R \) is the ideal gas constant (0.08206 L·atm/mol·K).
- \( T \) is the temperature in Kelvin (K).
1. **Convert Temperature to Kelvin:**
\[
T(K) = 35.6 + 273.15 = 308.75 \, K
\]
2. **Convert osmotic pressure to atm:**
\[
\pi(atm) = 599 \, mmHg \times \left(\frac{1 \, atm}{760 \, mmHg}\right) = 0.78816 \, atm
\]
3. **Calculate molarity (M):**
Molarity \( M \) can be found from:
\[
M = \frac{\pi}{R \cdot T}
\]
\[
M = \frac{0.78816}{0.08206 \times 308.75} = 0.0313 \, mol/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F600cf502-5061-4aa5-9b8a-58cefeae6855%2F2d93678b-400e-48f9-9b9d-e242642f77cd%2Fe9rptng_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining Molar Mass Based on Osmotic Pressure
**Question Prompt:**
If 2.98 g of a non-electrolyte produces an osmotic pressure of 599 mm Hg when dissolved in enough water to produce 183 mL of solution at 35.6 °C, what is the molar mass of the non-electrolyte? Report the answer to 3 significant figures and in g/mol.
**Instructions:**
Please type your answer in the space provided below. Note that moving to another question will save your current response.
[Insert answer box here]
**Additional Notes:**
This question is part of a quiz or homework assignment, so ensure to review your calculations and responses thoroughly. You can save your answers by proceeding to the next question.
**warning icon**: "Moving to another question will save this response."
**Navigation:**
Question 10 of 34
---
**Explanation for Calculation:**
To determine the molar mass of the non-electrolyte, you need to use the formula for osmotic pressure:
\[
\pi = i \cdot M \cdot R \cdot T
\]
Where:
- \( \pi \) is the osmotic pressure.
- \( i \) is the van't Hoff factor (which is 1 for non-electrolytes).
- \( M \) is the molarity of the solution.
- \( R \) is the ideal gas constant (0.08206 L·atm/mol·K).
- \( T \) is the temperature in Kelvin (K).
1. **Convert Temperature to Kelvin:**
\[
T(K) = 35.6 + 273.15 = 308.75 \, K
\]
2. **Convert osmotic pressure to atm:**
\[
\pi(atm) = 599 \, mmHg \times \left(\frac{1 \, atm}{760 \, mmHg}\right) = 0.78816 \, atm
\]
3. **Calculate molarity (M):**
Molarity \( M \) can be found from:
\[
M = \frac{\pi}{R \cdot T}
\]
\[
M = \frac{0.78816}{0.08206 \times 308.75} = 0.0313 \, mol/L
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