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 whichwere 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 1Sample 2AverageStated 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 m1J=1NmR-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 sample0.050 gSecond sampleWeight of empty capsule + cupWeight of antacid + capsule + cup0.050 g0.171 g0.177 gWeight of antacid used (g)Water level before reaction48.15 mL48.70 mLWater level after reaction22.85 mL23.30 mLVolume of CO liberated (ml.)Volume of CO liberated (m')Lab temperature20°C - 293.15KAtmospherie pressure (Potal) - 765.06mm HgPH20 at lab temperature 17.5mm HgPCO2=747.56mm HgDemonstrator'sInitialsTheory:In this experiment, a weighed sample of antacid compound is reacted with 6 molLHCl to produce carbon dioxide (CO,) in a closed vessel. The following chemicalprocess takes place:Antacid + HCIsalt + H;0+ CO: (g)Obviously the above is not a balanced chemical equation. This process is carried out atatmospheric pressure and room temperature. The volume of gas generated is determined bymeasuring the volume of water displaced (pushed down) using a gas-measuring burette. Theamount of CO, corresponding to the measured volume is calculated using the idealgas law (PV- nRT). The composition of the antacid compound is deduced from this andexpressed as either weight % of NaHCO, or weight % of CACO, depending on which of thesethe used antacid contains.The ideal gas law is used as follows to calculate the amount of liberated COPV = nRTwe want to calculate the number of moles of carbon dioxide produced in thereaction so we re-arrange the equation so thatn- PVRTn(CO.) - P(CO:) x V (CO.)RTIn 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. Thismust be corrected, using Dalton's law of partial pressures as indicated, for thecontribution 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 preparation3a.Antacid mixtures are provided. Pick one. Working in pairs, students will analyse thistwice. The mixture has the following stated composition (weight percent)::Product H% compositionProduct Q% compositionNaHCO,75.3CaCO335.3sucrose19.7kaolin1.9glucose3.9Mg trisilicate1.9реррermint0.42 - 1.1рерреrmintnot statedglucosenot stated3b.It is necessary to choose a sample mass such that the volume of CO2 generated doesnot exceed the capacity of the gas burettes.For Product H use 0.10 -0.13 gFor product Q use 0.20 - 0.25 g.

Question

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 whichwere 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 1Sample 2AverageStated 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 m1J=1NmR-8.314 J mol&#34; K (to be used when the units of Pare N m, Vare m' and Tare K)Antacid used (Circle one)First sample0.050 gSecond sampleWeight of empty capsule + cupWeight of antacid + capsule + cup0.050 g0.171 g0.177 gWeight of antacid used (g)Water level before reaction48.15 mL48.70 mLWater level after reaction22.85 mL23.30 mLVolume of CO liberated (ml.)Volume of CO liberated (m')Lab temperature20°C - 293.15KAtmospherie pressure (Potal) - 765.06mm HgPH20 at lab temperature 17.5mm HgPCO2=747.56mm HgDemonstrator'sInitialsTheory:In this experiment, a weighed sample of antacid compound is reacted with 6 molLHCl to produce carbon dioxide (CO,) in a closed vessel. The following chemicalprocess takes place:Antacid + HCIsalt + H;0+ CO: (g)Obviously the above is not a balanced chemical equation. This process is carried out atatmospheric pressure and room temperature. The volume of gas generated is determined bymeasuring the volume of water displaced (pushed down) using a gas-measuring burette. Theamount of CO, corresponding to the measured volume is calculated using the idealgas law (PV- nRT). The composition of the antacid compound is deduced from this andexpressed as either weight % of NaHCO, or weight % of CACO, depending on which of thesethe used antacid contains.The ideal gas law is used as follows to calculate the amount of liberated COPV = nRTwe want to calculate the number of moles of carbon dioxide produced in thereaction so we re-arrange the equation so thatn- PVRTn(CO.) - P(CO:) x V (CO.)RTIn 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. Thismust be corrected, using Dalton's law of partial pressures as indicated, for thecontribution 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&#34;;- room temperature, to be expressed in kelvin (K).Part 3: Sample preparation3a.Antacid mixtures are provided. Pick one. Working in pairs, students will analyse thistwice. The mixture has the following stated composition (weight percent)::Product H% compositionProduct Q% compositionNaHCO,75.3CaCO335.3sucrose19.7kaolin1.9glucose3.9Mg trisilicate1.9реррermint0.42 - 1.1рерреrmintnot statedglucosenot stated3b.It is necessary to choose a sample mass such that the volume of CO2 generated doesnot exceed the capacity of the gas burettes.For Product H use 0.10 -0.13 gFor product Q use 0.20 - 0.25 g.

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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?