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IMOLK Data, Trial 2 Ideal Gas Law-PV=nRT Molarity of HCI (M): Data, Trial 1 3.00M 3.00 M Volume of HCI (ml): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 22.5°C Temperature (°C): 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt: Mg + 2 HCl 1MgCl₂ + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water. (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R=

IMOLK Data, Trial 2 Ideal Gas Law-PV=nRT Molarity of HCI (M): Data, Trial 1 3.00M 3.00 M Volume of HCI (ml): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 22.5°C Temperature (°C): 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt: Mg + 2 HCl 1MgCl₂ + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water. (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R=

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
Chapter5: Gases
Section: Chapter Questions
Problem 133AE
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Accepted value R= 0.0821 Latm/mol K Ideal Gas Law - PV=nRT Data, Trial 1 Data, Trial 2 Molarity of HCI (M): 3.00M 3.00 M Volume of HCI (mL): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 Temperature (°C): 22.5°C 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt I Mg + 2 HCl → | MgCl2 + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R =
Transcribed Image Text:Accepted value R= 0.0821 Latm/mol K Ideal Gas Law - PV=nRT Data, Trial 1 Data, Trial 2 Molarity of HCI (M): 3.00M 3.00 M Volume of HCI (mL): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 Temperature (°C): 22.5°C 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt I Mg + 2 HCl → | MgCl2 + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R =
Calculations (Show all your work for trial one on the bottom of the page or on the back!) 1. The calculation for R hinges on the assumption that Mg is the limiting reagent. Show the calculations that demonstrate this for Trial 1. Also be sure to explain in words how your calculations prove the limiting reagent. 2. Prior to placing the eudiometer tube into the equilibration chamber, is the pressure inside the tube greater than or less than the pressure outside the tube. Explain your logic.
Transcribed Image Text:Calculations (Show all your work for trial one on the bottom of the page or on the back!) 1. The calculation for R hinges on the assumption that Mg is the limiting reagent. Show the calculations that demonstrate this for Trial 1. Also be sure to explain in words how your calculations prove the limiting reagent. 2. Prior to placing the eudiometer tube into the equilibration chamber, is the pressure inside the tube greater than or less than the pressure outside the tube. Explain your logic.
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