Hello, i'm trying to calculate theoretical pressure and I thought I did it right but I don't think I did and I was wondering if you could tell me if it's right or not so I can continue on with my homework. (It says to keep in mind my answers for a and b, and I didn't use B in my calculation so I'm thinking something is wrong, because what i'm trying to continue on depends on this answer. **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.- All sample calculations associated with the spreadsheet are **MUST** be completed in Q#1 of the Post-Lab to receive credit for the spreadsheet.---**1. Sample calculations using 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)\[ 0.112 \, \text{g Na}_2\text{CO}_3 \times \frac{1 \, \text{mol Na}_2\text{CO}_3}{105.99 \, \text{g Na}_2\text{CO}_3} \times \frac{1 \, \text{mol CO}_2}{1 \, \text{mol Na}_2\text{CO}_3} = 0.001056 \, \text{mol CO}_2 \]b. **Calculate the theoretical mole quantity of carbon dioxide gas produced from 5.0 mL of 1.0 M HCl aqueous solution.**\[ \frac{1.0 \, \text{mol HCl}}{1 \, \text{L}} \times 5.0 \, \text{mL} \times \frac{1}{1000 \, \text{mL}} \times \frac{1 \, \text{mol

Answered: Image /qna-images/answer/04f44bd3-7910-4665-89a5-782743b8cef3.jpghey as the column b says consider this co2 as ideal gas not real gas ,if you treat co2 as real gas than value of a and b are needed so only pv=nrt will be used here,, second you have calculated wrong numbers of mole of co2 so correct it.