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Calculate the data fill in the table in pic 1 and calculation question based on the general information given in pic 2. Thank you for helping！

Calculate the data fill in the table in pic 1 and calculation question based on the general information given in pic 2. Thank you for helping！

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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Calculate the data fill in the table in pic 1 and calculation question based on the general information given in pic 2. Thank you for helping！
The following information may be of value: 1 mm Hg = 133.3 N m²² (Pa) 0°C = 273.15 K 1J = 1 N m 1 mL = 1 x 10-6 m3 R= 8.314 J mol K (to be used when the units of P are N m2, V are m³ and T are K) Antacid used (Circle one) Q First sample Second sample Weight of empty capsule + cup 0.050 g 0.050 g Weight of antacid + capsule + cup 0.171 g 0.177 g Weight of antacid used (g) Water level before reaction 48.15 mL 48.70 mL Water level after reaction 22.85 mL 23.30 mL Volume of CO liberated (mL) Volume of CO2 liberated (m³) Lab temperature 20 °C = 293.15 K %3D Atmospheric pressure (Ptotal) 765.06 mm Hg PH2O at lab temperature = 17.5 mm Hg PCO2 = 747.56 mm Hg Demonstrator's Initials Calculations Write a balanced equation for (i) the reaction of NaHCO; (which is in product H) with hydrochloric acid, and (ii) the reaction of CaCO; (in product Q) with hydrochloric acid. (i) (ii)
Transcribed Image Text:The following information may be of value: 1 mm Hg = 133.3 N m²² (Pa) 0°C = 273.15 K 1J = 1 N m 1 mL = 1 x 10-6 m3 R= 8.314 J mol K (to be used when the units of P are N m2, V are m³ and T are K) Antacid used (Circle one) Q First sample Second sample Weight of empty capsule + cup 0.050 g 0.050 g Weight of antacid + capsule + cup 0.171 g 0.177 g Weight of antacid used (g) Water level before reaction 48.15 mL 48.70 mL Water level after reaction 22.85 mL 23.30 mL Volume of CO liberated (mL) Volume of CO2 liberated (m³) Lab temperature 20 °C = 293.15 K %3D Atmospheric pressure (Ptotal) 765.06 mm Hg PH2O at lab temperature = 17.5 mm Hg PCO2 = 747.56 mm Hg Demonstrator's Initials Calculations Write a balanced equation for (i) the reaction of NaHCO; (which is in product H) with hydrochloric acid, and (ii) the reaction of CaCO; (in product Q) with hydrochloric acid. (i) (ii)
Theory: In this experiment, a weighed sample of antacid compound is reacted with 6 molL1 HCl to produce carbon dioxide (CO2) in a closed vessel. The following chemical process takes place: Antacid + HCI salt + H;O + CO2 (g) Obviously the above is not a balanced chemical equation. This process is carried out at atmospheric pressure and room temperature. The volume of gas generated is determined by measuring the volume of water displaced (pushed down) using a gas-measuring burette. The amount of CO, corresponding to the measured volume is calculated using the ideal gas law (PV= nRT). The composition of the antacid compound is deduced from this and expressed as either weight % of NaHCO; or weight % of CaCO3, depending on which of these the used antacid contains. The ideal gas law is used as follows to calculate the amount of liberated CO2: PV = nRT we want to calculate the number of moles of carbon dioxide produced in the reaction so we re-arrange the equation so that n = PV n (CO2) = P (CO,) x V (CÓ ,) RT In using this equation: NCO2 = moles of CO,(g) produced from the known mass of antacid: P CO2 = (P atmosphere - PH,O) is the pressure due to CO2(g) expressed in N m2 (Pa). The total pressure of the new volume of gas is equal to the atmospheric pressure. This must be corrected, using Dalton's law of partial pressures as indicated, for the contribution due to the vapour pressure of water (Appendix 4); V = volume of CO:(g), to be expressed in SI units (m³); R = gas constant = 8.314 J K' mol": T = room temperature, to be expressed in kelvin (K). Part 3: Sample preparation За. Antacid mixtures are provided. Pick one. Working in pairs, students will analyse this twice. The mixture has the following stated composition (weight percent): Product H % composition Product Q % composition NaHCO, 75.3 CACO3 35.3 sucrose 19.7 kaolin 1.9 glucose 3.9 Mg trisilicate 1.9 реppermint 0.42 – 1.1 реppermint not stated glucose not stated 3b. It is necessary to choose a sample mass such that the volume of CO2 generated does not exceed the capacity of the gas burettes. For Product H use 0.10 – 0.13 g For product Q use 0.20 – 0.25 g.
Transcribed Image Text:Theory: In this experiment, a weighed sample of antacid compound is reacted with 6 molL1 HCl to produce carbon dioxide (CO2) in a closed vessel. The following chemical process takes place: Antacid + HCI salt + H;O + CO2 (g) Obviously the above is not a balanced chemical equation. This process is carried out at atmospheric pressure and room temperature. The volume of gas generated is determined by measuring the volume of water displaced (pushed down) using a gas-measuring burette. The amount of CO, corresponding to the measured volume is calculated using the ideal gas law (PV= nRT). The composition of the antacid compound is deduced from this and expressed as either weight % of NaHCO; or weight % of CaCO3, depending on which of these the used antacid contains. The ideal gas law is used as follows to calculate the amount of liberated CO2: PV = nRT we want to calculate the number of moles of carbon dioxide produced in the reaction so we re-arrange the equation so that n = PV n (CO2) = P (CO,) x V (CÓ ,) RT In using this equation: NCO2 = moles of CO,(g) produced from the known mass of antacid: P CO2 = (P atmosphere - PH,O) is the pressure due to CO2(g) expressed in N m2 (Pa). The total pressure of the new volume of gas is equal to the atmospheric pressure. This must be corrected, using Dalton's law of partial pressures as indicated, for the contribution due to the vapour pressure of water (Appendix 4); V = volume of CO:(g), to be expressed in SI units (m³); R = gas constant = 8.314 J K' mol": T = room temperature, to be expressed in kelvin (K). Part 3: Sample preparation За. Antacid mixtures are provided. Pick one. Working in pairs, students will analyse this twice. The mixture has the following stated composition (weight percent): Product H % composition Product Q % composition NaHCO, 75.3 CACO3 35.3 sucrose 19.7 kaolin 1.9 glucose 3.9 Mg trisilicate 1.9 реppermint 0.42 – 1.1 реppermint not stated glucose not stated 3b. It is necessary to choose a sample mass such that the volume of CO2 generated does not exceed the capacity of the gas burettes. For Product H use 0.10 – 0.13 g For product Q use 0.20 – 0.25 g.
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