Question

help with remaining calculations please

Unknown sample no. C Trial I Trial 2 1. Mass of 2. Mass of generator + sample before reaction () 3. Inst s approval of apparatus C. Determination of Vol ume, Temperature, and Pressure of the Carbon Dioxide Gas 1. Initial reading of volume of water in CO.-collecting graduated cylinder (mL) 2. Final reading of volume of water in CO-collecting graduated cylinder (mL) 3. Volume of CO,(g) collected (L) 4. Temperature of water C) 5. Barometric pressure (torr) 6. Vapor pressure of HO at"C (torr) 7. Pressure of dry CO,(g) (torr) 742. D. Amount of Carbon Dioxide Gas Evolved Mass of generator + sample after reaction (g) 2. Mass loss of generator = mass CO2 evolved (g) 3. Moles of CO, evolved (mol) 1. Experiment 13 187 Trial 1 Trial 2 E. Molar Volume of CO, Gas l. Pressure of dry CO.(g) (atm). See Part C.7. 2. Volume of CO.(g) at STP (L). See equation 13.4. 3. Molar volume of CO,(8) at STP (IUmol). See equation 13.2. 4. A verage molar volume of CO2(8) at STP (/mol) F. Percent CaCO, in Mixture 1. Moles of CaCO, in sample from mol CO2 generated (mol). See equation 13.1. 2. Mass of CaCO, in sample (g) 3. Mass of original sample (g) 4. Percent of CaCO3 in sample (%) 5. Average percent of CaCO3 in sample (%) Unknown sample no. Trial 1 Trial 2 .193 1. Mass of sample (g) 60.6L1 2. Mass of generator + sample before reaction e) 3. Instructor's approval of apparatus C. Determination of Volume, Temperature, and Pressure of the Carbon Dioxide Gas 1. Initial reading of volume of water in Co,-collecting graduated cylinder (mL) 2. Final reading of volume of water in CO,-collecting graduated cylinder (mL) 3. Volume of CO,(8) collected (L) 4. Temperature of water CC) 5. Barometric pressure (orr) 6. Vapor pressure of H,0 at C (torr) 7. Pressure of dry CO2(g) (torr) D. Amount of Carbon Dioxide Gas Evolved 1. Mass of generator+ sample after reaction (g) 2. Mass loss of generator mass CO2 evolved (&) 3. Moles of CO2 evolved (mol) Trial 2 E. Molar Volume of CO, Gas Trial 1 1. Pressure of dry CO2(g) (atm). See Part C.7 n tod 2. Volume of CO,(8) at STP (L). See equation 13.4. 3, Molar volume of cosuation 132. 4. Average molar volume of CO.(8) at STP (L/mol) F. Percent CaCO, in Mixture 1. Moles of CaCO, in sample from mol CO2 generated (mol). See equation 13.1. 2. Mass of CaCO, in sample (g) 3. Mass of original sample (g) 4, Percent of CaCO3 in sample (%) 5. Average percent of CaCO3 in sample (%) Molar Volume of Carbon The mass loss of the Caco, mixture is due to the mass of CO-(g) evolved in the Dioxide mass of CO, is converted to moles of CO, evolved. The volume of CO.(g). ent, is calculated at STP conditions (see equation 13.4). Knowing the number of moles and (13.2) collected over water under the temperature and pressure conditions of the experim the volume at STP, the molar volume of CO(g) is calculated - molar volume of CO Vco (STP) nco, Volume of Collected The CO(g) evolved in the reaction is collected by displacing an equal volume of water Carbon Dioxide at STPFigure 13.2 (top)]. Because the CO,(a) is bubbled through the water, it is considered Dalton's law of partial pressures: The total pressure, Pr, exerted by a mixture of gases is the sum of thepressure, Pt, in this volume is due to the combined pressures of the CO, gas, Pco, and individual pressures (called pressures) exerted by each of the constituent gases "wet," meaning that the volume occupied by the CO,(g) is also saturated with water vapor at the temperature of the water over which it is collected. Therefore, the total eadcoti t the water vapor, Puo The pressure of the dry CO, is calculated using Dalton's law of partial pressures. For carbon dioxide gas (13.3) The pressure of the water vapor, PHo: at the gas-collecting temperature (obtained from Appendix C) is subtracted from the total pressure of the gases, Pr, in the gas- collecting vessel. Experimentally, the total pressure of the gaseous mixture (CO2 + H,O) is adjusted to atmospheric pressure (Pr = Pam) by adjusting the water levels inside and outside the gas-collecting vessel to be equal [Figure 13.2 (bottom)). Atmos- P atm pheric pressure is read from the laboratory barometer Once the experimental values for the volume, pressure, and temperature of the CO (g) are determined, the volume of CO (g) at STP conditions is calculated using a combination of Boyle's law (P o 1/V) and Charles' law (V o T) with Pco, esp(torr) 760 torr 273 K wet' CO2 gas oolar ST (13.4) eplk) Boyle's law correction Charles' law correction P wet CO2 P atm This value is used in equation 13.2. In addition to the fact that the collected CO.(8) is wet, CO, also has an appreciable solubility in water. When the CO,(8) is bubbled through pure water, some of the CO dissolves in the water and is not measured as gas evolved in the reaction. To minimize with Figure 13.2 The collection of any loss of evolved CO, as a result of its water solubility, the water is saturated with CO2 gas over water lop) and the CO2 before the experiment is conducted. This saturation is completed with the addition pressure measurement of "wet of either sodium bicarbonate to slightly acidified water or an antacid tablet that evolves CO2 gas (bottom) CO2, such as Alka-Seltzer Percent Calcium Carbonate in Mixture By use of equation 13.1, once the moles of CO,(g) evolved in the reaction is known, the moles and mass of CaCO, in the heterogeneous mixture can be calculated. The per- cent CaCO, in the mixture is calculated by dividing this mass of CaCO, by that of the original mixture and multiplying by 100 mass of CaCO mass of mixture × 100 = % Caco, (13.5)

Answer 1

Cao qevutaalau l'evah 3 walitec) &('c ='273.is tal: 294-15K : 8.6 tor γ 612 18.6 do Mars lots G 0 661 GO.Go3 0.05G8 man co, evolve - 0.0562 Males 않 CO2 evolved - 。056 0.001t Volume 씩, coa (g) at STP- 23 3K at stp) a Teo expk)

CO, Ca molas volumo Vco, (STP) ncop 17.8503 Lmof Reacentaos Cacos in ninl a 0 O.193 0.(93