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

#1.a. You should not confuse with the term theoretical yield or something like that. It is the same thing like we calculate the simple or complex problems using basic concept. Just we need to Focus on basics and calculate the mole as usual. Decomposition of Na2CO3: Na2CO3 ➝ Na2O + CO2 No. of moles of Na2CO3 = given mass/molecular mass =0.1/106=0.00094 No. of moles of CO2 = No. of moles of Na2CO3 = 0.00094

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Chemistry

Stuck on how to solve for theoretical moles. (#1 a)

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

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