World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 41A
Related questions
Question
Stuck on how to solve for theoretical moles. (#1 a)
![**Post-laboratory Assignment**
**Excel Spreadsheet:**
**Part A:**
Use Excel to generate a spreadsheet with the following information:
| Column | Description |
|--------|-------------|
| A | Enter the measured masses of sodium carbonate from data page #1 |
| B | Theoretical Moles CO₂(g) – Using stoichiometry, calculate the theoretical number of moles of CO₂ that can be produced from each reactant entry. |
| C | Theoretical Pressure CO₂(g) – Using the ideal gas law, measured volume, and temperature, calculate the theoretical pressure of CO₂(g) that can be produced from the theoretical moles of CO₂(g) in column B. |
| D | Actual measured pressures of carbon dioxide gas produced from data page #1 |
- On your Excel spreadsheet, circle the mass of sodium carbonate in column A for when the limiting reactant changes. Compare the values in column B to the answer for #1b below.
**Sample calculations associated with the spreadsheet must be completed in QH1 of the Post-Lab to receive credit for the spreadsheet.**
---
**Sample Calculations:**
Use the quantities measured in the lab and the ideal gas law.
**Part A**
a. **Calculate the theoretical number of moles of carbon dioxide gas produced using your measured mass of sodium carbonate for the 0.100 grams of Na₂CO₃. (Sample calculation for column B)**
\[
0.1129 \, \text{Na}_2\text{CO}_3 \times \frac{1 \, \text{mol Na}_2\text{CO}_3}{105.99 \, \text{g Na}_2\text{CO}_3} \times \frac{1 \, \text{mol CO}_2}{1 \, \text{mol Na}_2\text{CO}_3} = 0.001056 \, \text{mol CO}_2
\]
b. **Calculate the theoretical mole quantity of carbon dioxide gas produced from 5.0 mL of 1.0 M HCl aqueous solution.**
\[
1.0 \, \text{M HCl} \times \frac{5.0 \, \text{mL}}{1} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} \times \frac{1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F448f7483-8a1e-4f39-ab0f-11fa3d239fa4%2Fccb80249-8b5d-488e-aa8a-6f73df198eb5%2Fee280g.jpeg&w=3840&q=75)
Transcribed Image Text:**Post-laboratory Assignment**
**Excel Spreadsheet:**
**Part A:**
Use Excel to generate a spreadsheet with the following information:
| Column | Description |
|--------|-------------|
| A | Enter the measured masses of sodium carbonate from data page #1 |
| B | Theoretical Moles CO₂(g) – Using stoichiometry, calculate the theoretical number of moles of CO₂ that can be produced from each reactant entry. |
| C | Theoretical Pressure CO₂(g) – Using the ideal gas law, measured volume, and temperature, calculate the theoretical pressure of CO₂(g) that can be produced from the theoretical moles of CO₂(g) in column B. |
| D | Actual measured pressures of carbon dioxide gas produced from data page #1 |
- On your Excel spreadsheet, circle the mass of sodium carbonate in column A for when the limiting reactant changes. Compare the values in column B to the answer for #1b below.
**Sample calculations associated with the spreadsheet must be completed in QH1 of the Post-Lab to receive credit for the spreadsheet.**
---
**Sample Calculations:**
Use the quantities measured in the lab and the ideal gas law.
**Part A**
a. **Calculate the theoretical number of moles of carbon dioxide gas produced using your measured mass of sodium carbonate for the 0.100 grams of Na₂CO₃. (Sample calculation for column B)**
\[
0.1129 \, \text{Na}_2\text{CO}_3 \times \frac{1 \, \text{mol Na}_2\text{CO}_3}{105.99 \, \text{g Na}_2\text{CO}_3} \times \frac{1 \, \text{mol CO}_2}{1 \, \text{mol Na}_2\text{CO}_3} = 0.001056 \, \text{mol CO}_2
\]
b. **Calculate the theoretical mole quantity of carbon dioxide gas produced from 5.0 mL of 1.0 M HCl aqueous solution.**
\[
1.0 \, \text{M HCl} \times \frac{5.0 \, \text{mL}}{1} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} \times \frac{1
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