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Please demonstrate how to do question 1 parts a, b, and c. You do not need to do them all, simply walk me through on how to do the calculations.

Please demonstrate how to do question 1 parts a, b, and c. You do not need to do them all, simply walk me through on how to do the calculations.

Chemistry
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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Please demonstrate how to do question 1 parts a, b, and c. You do not need to do them all, simply walk me through on how to do the calculations.
Part A: Varied Masses of Sodium Carbonate * Reaction flask measured volume: dsevo 271.62ML レニ Concentration of HCl on the bottle_ o 1-OM Room Temperature_20.5°c /69.S OF (a) (e) (d) Final (b) (c) Actual Volume of Initial Pressure of Approx. Sample Mass of Sedium car bunaA Metal pressure in the flask CO2(g) (d – c) Acid Pressure in mass Added the flask 73.7 mm Hg 574.4 mm' 1 0.100 g •lo2g S.OmL 500.7 _mm Hg 2 mm .1539 0.150 g 5.0 mL 3 0.200 g 623.4 23.1 . 2009 SOML 500.3 nm Hg 4 0.250 g 0-253 g S.0mL S0o.7 mm Hg 630.3 mm Ha (29.6 mm Hg 0.300 g 0.305g 694.4 193.5 500, 9 mm Hg mm Hg 6 0.350 g 0.3519 714.4 214.0 mmitg 5.0mL 7 0.400 g 714.0 mm Hg .400 5.0mL 213.2 8. 0.450 g bo4519 soo. 9mmHg 78s,9 mmi4g 285.ommHg S.OML Rev. 10-13-21 JBT Page 11 2.
Transcribed Image Text:Part A: Varied Masses of Sodium Carbonate * Reaction flask measured volume: dsevo 271.62ML レニ Concentration of HCl on the bottle_ o 1-OM Room Temperature_20.5°c /69.S OF (a) (e) (d) Final (b) (c) Actual Volume of Initial Pressure of Approx. Sample Mass of Sedium car bunaA Metal pressure in the flask CO2(g) (d – c) Acid Pressure in mass Added the flask 73.7 mm Hg 574.4 mm' 1 0.100 g •lo2g S.OmL 500.7 _mm Hg 2 mm .1539 0.150 g 5.0 mL 3 0.200 g 623.4 23.1 . 2009 SOML 500.3 nm Hg 4 0.250 g 0-253 g S.0mL S0o.7 mm Hg 630.3 mm Ha (29.6 mm Hg 0.300 g 0.305g 694.4 193.5 500, 9 mm Hg mm Hg 6 0.350 g 0.3519 714.4 214.0 mmitg 5.0mL 7 0.400 g 714.0 mm Hg .400 5.0mL 213.2 8. 0.450 g bo4519 soo. 9mmHg 78s,9 mmi4g 285.ommHg S.OML Rev. 10-13-21 JBT Page 11 2.
Post-laboratory Assignment (page 1 of 4) Excel Spreadsheet: Part A: Room Use Excel to generate a spreadsheet with the following information. (d) rature Column ressre Enter the measured masses of sodium carbonate from data page #1 Theoretical Moles CO2(g) – Using stoichiometry, calculate the theoretical number of moles of CO2 that can be produced from each reactant entry. 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. A В C 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) 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 and the quantities measured in the lab for the 0.100 g Na2CO3 trial. (hint: consider your answers from a & b when doing this calculation.) ev. 10-13-21 BT Page |13
Transcribed Image Text:Post-laboratory Assignment (page 1 of 4) Excel Spreadsheet: Part A: Room Use Excel to generate a spreadsheet with the following information. (d) rature Column ressre Enter the measured masses of sodium carbonate from data page #1 Theoretical Moles CO2(g) – Using stoichiometry, calculate the theoretical number of moles of CO2 that can be produced from each reactant entry. 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. A В C 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) 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 and the quantities measured in the lab for the 0.100 g Na2CO3 trial. (hint: consider your answers from a & b when doing this calculation.) ev. 10-13-21 BT Page |13
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