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Data Table Use the following table to record your data for each trial. Trial 1 Atmospheric pressure Mass of magnesium metal Volume of 6 M hydrochloric acid Volume of molecular hydrogen gas Water temperature Partial pressure of water (at above temperature) Calculations Do the following calculations for each trial. Trial 2 19.0c 16.48tor Trial 3 29.39in29.39in29.39in 0.085g 0.0779 0.08.39 10.0mL 10.0m 10.0mL 86.63mL77.50ml 79.60m 19.0c 19.0°c Pressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube. Using the measured atmospheric pressure and the partial pressure of water vapor (determined from the temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial. Trial 1: Patm = 29.39inHgx254cmx10mm=746.506mmHg Moles of H,gas: Using the molar mass of magnesium and the balanced equation for the reaction you have just observed, calculate the moles of molecular hydrogen that should have been formed. This calculation assumes that the magnesium was pure and was completely consumed by the hydrochloric acid, and that no H, was lost in the process (i.e., it assumes a 100% yield of hydrogen gas).

Data Table Use the following table to record your data for each trial. Trial 1 Atmospheric pressure Mass of magnesium metal Volume of 6 M hydrochloric acid Volume of molecular hydrogen gas Water temperature Partial pressure of water (at above temperature) Calculations Do the following calculations for each trial. Trial 2 19.0c 16.48tor Trial 3 29.39in29.39in29.39in 0.085g 0.0779 0.08.39 10.0mL 10.0m 10.0mL 86.63mL77.50ml 79.60m 19.0c 19.0°c Pressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube. Using the measured atmospheric pressure and the partial pressure of water vapor (determined from the temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial. Trial 1: Patm = 29.39inHgx254cmx10mm=746.506mmHg Moles of H,gas: Using the molar mass of magnesium and the balanced equation for the reaction you have just observed, calculate the moles of molecular hydrogen that should have been formed. This calculation assumes that the magnesium was pure and was completely consumed by the hydrochloric acid, and that no H, was lost in the process (i.e., it assumes a 100% yield of hydrogen gas).

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Data Table Use the following table to record your data for each trial. Trial 1 Atmospheric pressure Mass of magnesium metal Volume of 6 M hydrochloric acid Volume of molecular hydrogen gas Name: Macy Hufford Water temperature Partial pressure of water (at above temperature) Calculations Do the following calculations for each trial. Trial 2 19.0c 16.48tom Trial 3 29.39inH29.39in29.39in 0.085g 0.0779 0.0839 110.0mL 10.0m 10.00L 86.63mL77.50ml 79.600 19.0c 19.0c Pressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube. Using the measured atmospheric pressure and the partial pressure of water vapor (determined from the temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial. Trial 1: Patm=29,39inHgx254cmx10mm-746.506mmHg 1in Moles of H,gas: Using the molar mass of magnesium and the balanced equation for the reaction you have just observed, calculate the moles of molecular hydrogen that should have been formed. This calculation assumes that the magnesium was pure and was completely consumed by the hydrochloric acid, and that no H₂ was lost in the process (i.e., it assumes a 100% yield of hydrogen gas).
Transcribed Image Text:Data Table Use the following table to record your data for each trial. Trial 1 Atmospheric pressure Mass of magnesium metal Volume of 6 M hydrochloric acid Volume of molecular hydrogen gas Name: Macy Hufford Water temperature Partial pressure of water (at above temperature) Calculations Do the following calculations for each trial. Trial 2 19.0c 16.48tom Trial 3 29.39inH29.39in29.39in 0.085g 0.0779 0.0839 110.0mL 10.0m 10.00L 86.63mL77.50ml 79.600 19.0c 19.0c Pressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube. Using the measured atmospheric pressure and the partial pressure of water vapor (determined from the temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial. Trial 1: Patm=29,39inHgx254cmx10mm-746.506mmHg 1in Moles of H,gas: Using the molar mass of magnesium and the balanced equation for the reaction you have just observed, calculate the moles of molecular hydrogen that should have been formed. This calculation assumes that the magnesium was pure and was completely consumed by the hydrochloric acid, and that no H₂ was lost in the process (i.e., it assumes a 100% yield of hydrogen gas).
San Diego Miramar College | Chem 152L Laboratory Calculations (continued) Use the ideal gas law, the pressure of H, and moles of H, calculated above, along with the volume and temperature from your data table, to calculate the ideal gas constant (R) for each trial. Calculate the average value of R for your three trials. Calculate the % error between your average and the literature value of R = 0.08206 L-atm/K mol.
Transcribed Image Text:San Diego Miramar College | Chem 152L Laboratory Calculations (continued) Use the ideal gas law, the pressure of H, and moles of H, calculated above, along with the volume and temperature from your data table, to calculate the ideal gas constant (R) for each trial. Calculate the average value of R for your three trials. Calculate the % error between your average and the literature value of R = 0.08206 L-atm/K mol.
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