alculations of Unknown % artial Pressure of CO2 (mmHg) ortial Pressure of CO2 (atm) oles of CO2 loles of NaCO3 lass of NaCO3 grams of NaCO3 verage % of NaCO3 TD 756.2 756.2
alculations of Unknown % artial Pressure of CO2 (mmHg) ortial Pressure of CO2 (atm) oles of CO2 loles of NaCO3 lass of NaCO3 grams of NaCO3 verage % of NaCO3 TD 756.2 756.2
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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Hi I am having trouble finding the rest of the data for the blank excel boxes. The given date will be on the right side of the excel photo, I just need to find the answers for the excel table on the left. I have also attached the formulas needed to find them. Thank you.
![**Calculations of Unknown %**
**Trial 1**
1. **Partial Pressure of CO2 (mmHg):** 756.2
2. **Partial Pressure of CO2 (atm):** [Not provided]
3. **Moles of CO2:** [Not provided]
4. **Moles of NaCO3:** [Not provided]
5. **Mass of NaCO3 grams:** [Not provided]
6. **% of NaCO3:** [Not provided]
7. **Average % of NaCO3:** [Not provided]
8. **STD (Standard Deviation):** [Not provided]
---
**Trial 2**
1. **Partial Pressure of CO2 (mmHg):** 756.2
2. **Partial Pressure of CO2 (atm):** [Not provided]
3. **Moles of CO2:** [Not provided]
4. **Moles of NaCO3:** [Not provided]
5. **Mass of NaCO3 grams:** [Not provided]
6. **% of NaCO3:** [Not provided]
7. **Average % of NaCO3:** [Not provided]
8. **STD (Standard Deviation):** [Not provided]
---
**Unknown Number**
- **Mass of Unknown before Rxn (g):**
- Trial 1: 1.03
- Trial 2: 1.009
- **Initial Volume in Graduated Cyl (mL):**
- Trial 1: 203
- Trial 2: 200
- **Final Volume in Graduated Cyl (mL):**
- Trial 1: 340
- Trial 2: 333
- **Change in Volume CO3 (mL):**
- Trial 1: [Not calculated]
- Trial 2: [Not calculated]
- **Temp of CO2 Celsius:**
- Trial 1: 24
- Trial 2: 24
- **Pressure of Lab (mmHg):**
- Trial 1: 761.1
- Trial 2: 761.1
- **Vap Press H2O:**
- Trial 1: 4.9
- Trial 2: 4.9
**Diagram Explanation:**
This table outlines the experimental data and conditions for two trials investigating an unknown compound. Key variables measured](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf266520-407e-4b51-839c-e1d92d759be6%2F00c1eb0e-8426-4aca-94c5-b0f03101fa60%2F7ejykc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Calculations of Unknown %**
**Trial 1**
1. **Partial Pressure of CO2 (mmHg):** 756.2
2. **Partial Pressure of CO2 (atm):** [Not provided]
3. **Moles of CO2:** [Not provided]
4. **Moles of NaCO3:** [Not provided]
5. **Mass of NaCO3 grams:** [Not provided]
6. **% of NaCO3:** [Not provided]
7. **Average % of NaCO3:** [Not provided]
8. **STD (Standard Deviation):** [Not provided]
---
**Trial 2**
1. **Partial Pressure of CO2 (mmHg):** 756.2
2. **Partial Pressure of CO2 (atm):** [Not provided]
3. **Moles of CO2:** [Not provided]
4. **Moles of NaCO3:** [Not provided]
5. **Mass of NaCO3 grams:** [Not provided]
6. **% of NaCO3:** [Not provided]
7. **Average % of NaCO3:** [Not provided]
8. **STD (Standard Deviation):** [Not provided]
---
**Unknown Number**
- **Mass of Unknown before Rxn (g):**
- Trial 1: 1.03
- Trial 2: 1.009
- **Initial Volume in Graduated Cyl (mL):**
- Trial 1: 203
- Trial 2: 200
- **Final Volume in Graduated Cyl (mL):**
- Trial 1: 340
- Trial 2: 333
- **Change in Volume CO3 (mL):**
- Trial 1: [Not calculated]
- Trial 2: [Not calculated]
- **Temp of CO2 Celsius:**
- Trial 1: 24
- Trial 2: 24
- **Pressure of Lab (mmHg):**
- Trial 1: 761.1
- Trial 2: 761.1
- **Vap Press H2O:**
- Trial 1: 4.9
- Trial 2: 4.9
**Diagram Explanation:**
This table outlines the experimental data and conditions for two trials investigating an unknown compound. Key variables measured
![### Transcription and Explanation:
**Equation 8 Rearrangement for Partial Pressure of CO₂:**
\[ P_{CO_2} = P_{lab} - P_{H_2O} \]
(Equation 9)
This indicates that the partial pressure of CO₂ can be determined by subtracting the vapor pressure of water (\(P_{H_2O}\)) from the total pressure in the lab (\(P_{lab}\)).
**Conversion to Moles Using Ideal Gas Law:**
Once the partial pressure of CO₂ is known, it can be used to calculate the moles of CO₂ gas produced using the ideal gas law:
\[ n_{CO_2} = \frac{P_{CO_2} \times V_{CO_2}}{R \times T_{lab}} \]
(Equation 10)
Where:
- \( n_{CO_2} \) is the number of moles of CO₂.
- \( V_{CO_2} \) is the volume of CO₂.
- \( R \) is the ideal gas constant.
- \( T_{lab} \) is the temperature in the lab.
**Conversion to Grams of Sodium Carbonate:**
The moles of CO₂ produced can be converted to grams of sodium carbonate (\(Na_2CO_3\)) as follows:
\[ \text{mass } Na_2CO_3 = n_{CO_2} \times \left( \frac{1 \text{ mole } Na_2CO_3}{1 \text{ mole } CO_2} \right) \times \left( \frac{105.97 \text{ g}}{1 \text{ mole } Na_2CO_3} \right) \]
(Equation 11)
**Calculation of Mass Percent:**
The mass percent of \(Na_2CO_3\) in the unknown sample is calculated using:
\[ \text{mass \% } Na_2CO_3 = \left( \frac{\text{mass } Na_2CO_3}{\text{total unknown mass}} \right) \times 100 \]
(Equation 12)
**Instructions for Experimental Data Analysis:**
From the data collected from two trials, calculate the mass percent of \(Na_2CO_3\) in the unknown sample. Perform all calculations carefully, paying special attention to](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf266520-407e-4b51-839c-e1d92d759be6%2F00c1eb0e-8426-4aca-94c5-b0f03101fa60%2Feg47zi7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Transcription and Explanation:
**Equation 8 Rearrangement for Partial Pressure of CO₂:**
\[ P_{CO_2} = P_{lab} - P_{H_2O} \]
(Equation 9)
This indicates that the partial pressure of CO₂ can be determined by subtracting the vapor pressure of water (\(P_{H_2O}\)) from the total pressure in the lab (\(P_{lab}\)).
**Conversion to Moles Using Ideal Gas Law:**
Once the partial pressure of CO₂ is known, it can be used to calculate the moles of CO₂ gas produced using the ideal gas law:
\[ n_{CO_2} = \frac{P_{CO_2} \times V_{CO_2}}{R \times T_{lab}} \]
(Equation 10)
Where:
- \( n_{CO_2} \) is the number of moles of CO₂.
- \( V_{CO_2} \) is the volume of CO₂.
- \( R \) is the ideal gas constant.
- \( T_{lab} \) is the temperature in the lab.
**Conversion to Grams of Sodium Carbonate:**
The moles of CO₂ produced can be converted to grams of sodium carbonate (\(Na_2CO_3\)) as follows:
\[ \text{mass } Na_2CO_3 = n_{CO_2} \times \left( \frac{1 \text{ mole } Na_2CO_3}{1 \text{ mole } CO_2} \right) \times \left( \frac{105.97 \text{ g}}{1 \text{ mole } Na_2CO_3} \right) \]
(Equation 11)
**Calculation of Mass Percent:**
The mass percent of \(Na_2CO_3\) in the unknown sample is calculated using:
\[ \text{mass \% } Na_2CO_3 = \left( \frac{\text{mass } Na_2CO_3}{\text{total unknown mass}} \right) \times 100 \]
(Equation 12)
**Instructions for Experimental Data Analysis:**
From the data collected from two trials, calculate the mass percent of \(Na_2CO_3\) in the unknown sample. Perform all calculations carefully, paying special attention to
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