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Convert PCO: from mm Hg to N m (Pa) Using the ideal gas equation (PV = nRT), calculate the number of moles (n) of CO2 which were liberated by reaction of your antacid sample. (b) (c) How many moles of NaHCO/CaCO, are required to yield this number of moles of CO2?

Convert PCO: from mm Hg to N m (Pa) Using the ideal gas equation (PV = nRT), calculate the number of moles (n) of CO2 which were liberated by reaction of your antacid sample. (b) (c) How many moles of NaHCO/CaCO, are required to yield this number of moles of CO2?

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
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Please help me to complete the questions of pic 1, AND pic 2 is some relevant information. Need detailed calculation process and answers, thank you very much for your help！
(a) Convert PCO2 from mm Hg to N m2 (Pa) Using the ideal gas equation (PV = nRT), calculate the number of moles (n) of CO2 which were liberated by reaction of your antacid sample. (b) (c) How many moles of NaHCO:/CACO; are required to yield this number of moles of C02? (d) What mass (in grams) is this amount of NaHCO:/CaCO; equivalent to? (e) Calculate the weight percent of NaHCO3/CaCO; in the sample. Now fill in table summarizing your results for samples 1 and 2. wt % Sample 1 Sample 2 Average Stated weight percent of NaHCO3/CaCO; for your product (see Lab Manual):
Transcribed Image Text:(a) Convert PCO2 from mm Hg to N m2 (Pa) Using the ideal gas equation (PV = nRT), calculate the number of moles (n) of CO2 which were liberated by reaction of your antacid sample. (b) (c) How many moles of NaHCO:/CACO; are required to yield this number of moles of C02? (d) What mass (in grams) is this amount of NaHCO:/CaCO; equivalent to? (e) Calculate the weight percent of NaHCO3/CaCO; in the sample. Now fill in table summarizing your results for samples 1 and 2. wt % Sample 1 Sample 2 Average Stated weight percent of NaHCO3/CaCO; for your product (see Lab Manual):
The following information may be of value: 1 mm Hg - 133.3 Nm (Pa) 0°C = 273.15 K. I ml -1x 10 m 1J=1Nm R-8.314 J mol" K (to be used when the units of Pare N m, Vare m' and Tare K) Antacid used (Circle one) First sample 0.050 g Second sample Weight of empty capsule + cup Weight of antacid + capsule + cup 0.050 g 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 CO liberated (m') Lab temperature 20 °C - 293.15 K Atmospherie pressure (Potal) - 765.06 mm Hg PH20 at lab temperature 17.5 mm Hg PCO2=747.56 mm Hg Demonstrator's Initials Theory: In this experiment, a weighed sample of antacid compound is reacted with 6 molL HCl to produce carbon dioxide (CO,) in a closed vessel. The following chemical process takes place: Antacid + HCI salt + H;0+ CO: (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 CACO, depending on which of these the used antacid contains. The ideal gas law is used as follows to calculate the amount of liberated CO 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 RT n(CO.) - P(CO:) x V (CO.) RT In using this equation: nCO, = moles of CO:(g) produced from the known mass of antacid; P CO: = (Patmosphere - PH:0) is the pressure due to CO:(g) expressed in N m (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 (m'); = gas constant = 8.314 J K' mol "; - room temperature, to be expressed in kelvin (K). Part 3: Sample preparation 3a. 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 реррermint 0.42 - 1.1 рерреrmint 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:The following information may be of value: 1 mm Hg - 133.3 Nm (Pa) 0°C = 273.15 K. I ml -1x 10 m 1J=1Nm R-8.314 J mol" K (to be used when the units of Pare N m, Vare m' and Tare K) Antacid used (Circle one) First sample 0.050 g Second sample Weight of empty capsule + cup Weight of antacid + capsule + cup 0.050 g 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 CO liberated (m') Lab temperature 20 °C - 293.15 K Atmospherie pressure (Potal) - 765.06 mm Hg PH20 at lab temperature 17.5 mm Hg PCO2=747.56 mm Hg Demonstrator's Initials Theory: In this experiment, a weighed sample of antacid compound is reacted with 6 molL HCl to produce carbon dioxide (CO,) in a closed vessel. The following chemical process takes place: Antacid + HCI salt + H;0+ CO: (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 CACO, depending on which of these the used antacid contains. The ideal gas law is used as follows to calculate the amount of liberated CO 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 RT n(CO.) - P(CO:) x V (CO.) RT In using this equation: nCO, = moles of CO:(g) produced from the known mass of antacid; P CO: = (Patmosphere - PH:0) is the pressure due to CO:(g) expressed in N m (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 (m'); = gas constant = 8.314 J K' mol "; - room temperature, to be expressed in kelvin (K). Part 3: Sample preparation 3a. 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 реррermint 0.42 - 1.1 рерреrmint 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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