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...
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how do we find the average of the molar mass of these unkown liquid? how to express the water bath temperature in Kelvin?
Transcribed Image Text:**Experimental Data Table**
The table presents data from an experiment involving unknown substances across five trials. Each trial records several parameters:
1. **Mass of Flask, Boiling Stone, Foil Cap, and Unknown After Cooling (g)**:
- Unknown 1: Trial 1 (80.480 g), Trial 2 (81.021 g)
- Unknown 2: Trial 1 (86.081 g), Trial 2 (86.002 g)
- Unknown 3: Trial 1 (106.506 g), Trial 2 (106.540 g)
- Unknown 4: Trial 1 (105.975 g), Trial 2 (106.209 g)
- Unknown 5: Trial 1 (98.675 g), Trial 2 (99.628 g)
2. **Mass of Empty Flask, Boiling Stone, and Foil Cap (g)**:
- Unknown 1: 80.034 g
- Unknown 2: 85.868 g
- Unknown 3: 105.879 g
- Unknown 4: 105.509 g
- Unknown 5: 98.358 g
3. **Mass of Unknown (g)**:
- Unknown 1: Trial 1 (0.446 g), Trial 2 (0.477 g)
- Unknown 2: Trial 1 (0.213 g), Trial 2 (0.204 g)
- Unknown 3: Trial 1 (0.627 g), Trial 2 (0.615 g)
- Unknown 4: Trial 1 (0.466 g), Trial 2 (0.473 g)
- Unknown 5: Trial 1 (0.317 g), Trial 2 (0.33 g)
4. **Water Bath Temperature at Complete Vaporization (°C)**:
- Unknown 1: 100.0 °C
- Unknown 2: 99.0 °C, 100.0 °C
- Unknown 3: 101.0 °C
- Unknown 4: 103.0 °C, 102.0 °C
- Unknown 5: 100.0 °C, 99.0 °C
5. **Barometric Pressure (mmHg)**:
- Unknown 1: 770 mmHg
![**Calculations: (Show full calculations for one trial of your unknown)**
1. **Calculate the mass of the condensed liquid in the flask.**
(*See data at the end of the lab*)
2. **Next, express the water bath temperature in Kelvin.**
3. **Express the barometric pressure in atmospheres (atm), using the following conversion:**
\(1 \, \text{atm} = 760 \, \text{mmHg}\)
4. **Convert the volume of the flask from milliliters to liters, using the following conversion:**
\(1 \, \text{Liter} = 1000 \, \text{mL}\)
5. **Now, calculate the density of the vaporized unknown using the density equation:**
\(\text{Density} \, (\text{g/L}) = \frac{\text{mass}}{\text{volume}}\)
6. **Lastly, calculate the molar mass (MM) of the unknown solution using the following equation:**
\[ MM = \frac{d \times R \times T}{P} \]
7. **Calculate the average of the molar mass of the unknown liquid and identify the unknown from the list above.**
**Post Lab Questions:**
(Refer to the original document for detailed post-lab analysis and questions.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff7e0b628-1887-4036-8cfa-486903c53c1e%2Ffc6ae24e-d11f-4540-b68c-31bb2139e79f%2Fia7qwg7.jpeg&w=3840&q=75)
Transcribed Image Text:**Calculations: (Show full calculations for one trial of your unknown)**
1. **Calculate the mass of the condensed liquid in the flask.**
(*See data at the end of the lab*)
2. **Next, express the water bath temperature in Kelvin.**
3. **Express the barometric pressure in atmospheres (atm), using the following conversion:**
\(1 \, \text{atm} = 760 \, \text{mmHg}\)
4. **Convert the volume of the flask from milliliters to liters, using the following conversion:**
\(1 \, \text{Liter} = 1000 \, \text{mL}\)
5. **Now, calculate the density of the vaporized unknown using the density equation:**
\(\text{Density} \, (\text{g/L}) = \frac{\text{mass}}{\text{volume}}\)
6. **Lastly, calculate the molar mass (MM) of the unknown solution using the following equation:**
\[ MM = \frac{d \times R \times T}{P} \]
7. **Calculate the average of the molar mass of the unknown liquid and identify the unknown from the list above.**
**Post Lab Questions:**
(Refer to the original document for detailed post-lab analysis and questions.)
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