1. Perform the following calculations for Mg(s)a) Calculate the vapor pressure of water at the temperature of your experiment (see appendix 1)b) Calculate the pressure (in kPa) of the water column formed by the difference in the solution levels inside and outside the gas burette (i.e. convert from mm H2O to kPa)c) Calculate the pressure (bar) exerted by the hydrogen gas aloned) Calculate the number of moles of H2(g) Produced in the reaction of Mg(s) with HCl(aq), Mg(s) is the limiting reactant e) Calculate the value of the ideal gas constant, R (L bar mol-1 K-1)Appendix and numbers needed are added RAW DATALABORATORY REPORTMass of Mg(s)Final burette reading for Mg(s) procedureDifference in solution levels for Mg(s) procedureAtmospheric pressure, Patm (provided by lab instructor)Temperatureof trapped gas (provided by lab instructor)0.076977.42138102.518.5mLmm H₂OkPa°C APPENDIX 1 VAPOUR PRESSURE OF WATERTemp°℃0.01.02.03.04.05.06.07.08.09.010.011.012.013.014.015.016.0Table 3 - The vapor pressure of water from 0 to 105 °C at 1 degree intervalsTemp°C34.035.040.045.050.055.060.065.0PressuremmHg4.64.95.35.76.16.57.07.58.08.69.29.810.511.212.012.813.6kPa0.6130.6530.7060.7600.8130.8660.9331.001.071.151.231.311.401.491.601.711.81Temp°C17.018.019.020.021.022.023.024.025.026.027.028.029.030.031.032.033.0PressuremmHg14.515.516.517.518.719.821.122.423.825.226.728.330.031.833.735.737.7kPa1.932.072.202.332.492.642.812.993.173.363.563.774.004.244.494.765.0370.075.080.085.090.095.0100.0105.0PressuremmHg39.942.255.371.992.5118149188233289355434526634760906kPa5.325.627.379.5812.315.719.925.131.138.547.357.870.184.5101.3120.8FARLY INTERPOLATE USING A TABLEorder to estimate a value that lies between two data points in a table the process of linear interpolation c

As per the guidelines, we will solve the first three parts, if you need any other part to be solved…

1. Perform the following calculations for Mg(s) a) Calculate the vapor pressure of water at the temperature of your experiment (see appendix 1) b) Calculate the pressure (in kPa) of the water column formed by the difference in the solution levels inside and outside the gas burette (i.e. convert from mm H2O to kPa) c) Calculate the pressure (bar) exerted by the hydrogen gas alone d) Calculate the number of moles of H2(g) Produced in the reaction of Mg(s) with HCl(aq), Mg(s) is the limiting reactant e) Calculate the value of the ideal gas constant, R (L bar mol-1 K-1)

1. Perform the following calculations for Mg(s) a) Calculate the vapor pressure of water at the temperature of your experiment (see appendix 1) b) Calculate the pressure (in kPa) of the water column formed by the difference in the solution levels inside and outside the gas burette (i.e. convert from mm H2O to kPa) c) Calculate the pressure (bar) exerted by the hydrogen gas alone d) Calculate the number of moles of H2(g) Produced in the reaction of Mg(s) with HCl(aq), Mg(s) is the limiting reactant e) Calculate the value of the ideal gas constant, R (L bar mol-1 K-1)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.24QAP

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In Part B, you used a similar procedure to that of Part A to determine the mass percent of CaCO3 in an antacid tablet. The commercially accepted range of CaCO3 in an antacid tablet is 25–35% by mass. Miranda obtained the data below from her Part B trial: TRIAL PRESSURE (torr) MASS OF TABLET (g) TEMPERATURE (°C) VOLUME CO2 RECOVERED (mL) 1 750.5 0.5702 21.3 69.6 2 750.5 0.5622 21.2 68.2 Miranda determined her average % Recovery of CO2 to be 65.0% from Part A. Based on her data collected from Part A, was the average percent mass of CaCO3 in her antacid tablet within the commercially accepted range? Yes, her mass percent does fall within the commercially accepted range. No, her mass percent does not fall within the commercially accepted range.
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For PV = nRT to be valid, the gas has to act______________
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