Question

need help with #1 a-c

Post-laboratory Assignment (page 1 of 5) Excel Spreadsheet: Part A Use Excel to generate a spreadsheet with the following information. Column A Enter the measured masses of sodium carbonate from data page 1 B Using stoichiometry, calculate the theoretical number of moles of CO, that can be produced from each reactant entry. C 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 COrg). 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 lb below. All sample calculations associated with the spreadsheet are MUST be completed in Oll 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 NazCO. (Sample calculation for column B) b. Calculate the theoretical mole quantity of carbon dioxide gas produced from 5.0 mL of 1.0 M HCl aqueous solution. c. Calculate the theoretical pressure of carbon dioxide gas produced in the flask using the reaction conditions in the lab and the actual quantities reacted in the 0.100 g NagCO3 trial. Cev. 10-20-19

Answer 1

Part a.

Moles of Na2CO3 = 0.1 g/(106 g/mol) = 9.434*10^-6 mol

According to the following equation: Na2CO3 --$\Delta$--> Na2O + CO2(g)

The mole ratio Na2CO3:CO2 = 1:1

Therefore, the moles of CO2 produced = 9.434*10^-6 mol

Part b.

Na2CO3 + 2HCl ----> 2NaCl + CO2 + H2O

The mole ratio HCl:CO2 = 2:1

The moles of HCl = (5/1000) L * 1 mol/L = 0.005 mol

Therefore, the moles of CO2 produced = 0.005/2 = 0.0025 mol

Part c.

According to ideal gas equation:

PV = nRT

i.e. P * (300/1000) L =  9.434*10^-6 mol * 0.0821 L.atm/mol.K * (21.5+273) K

Therefore, the pressure of CO2 (P) = 7.6*10^-4 atm