Mass of Mg: .0403g
Room Pressure: 3.021 Hg x 2.45cm/1in x 10mm/1cm
Volume of H2 gas (convert to liters): 63.5 ml--->.635L
Room Temperature: 297.9 C°
Water vapor Pressure (atm): 23.8 - 760= 0.0313
1. Determine the partial pressure of H2 by subtracting the water vapor pressure from the room pressure.
2. Using the partial pressure for H2 from question #1, use the ideal gas law to determine the number of moles of H2 actually collected
3. Determine the theoretical yield, in moles pf H2, based on the Mg being the limiting reactant.
4. Determine the % yield for H2
Note: I am new to the forum. I just wanted to confirm that I have attempted these and have tried to get pictures of my work but was unable to do so. Any help is greatly appreciated. Thank You
Room Pressure: 3.021 Hg x 2.45cm/1in x 10mm/1cm
Volume of H2 gas (convert to liters): 63.5 ml--->.635L
Room Temperature: 297.9 C°
Water vapor Pressure (atm): 23.8 - 760= 0.0313
1. Determine the partial pressure of H2 by subtracting the water vapor pressure from the room pressure.
2. Using the partial pressure for H2 from question #1, use the ideal gas law to determine the number of moles of H2 actually collected
3. Determine the theoretical yield, in moles pf H2, based on the Mg being the limiting reactant.
4. Determine the % yield for H2
Note: I am new to the forum. I just wanted to confirm that I have attempted these and have tried to get pictures of my work but was unable to do so. Any help is greatly appreciated. Thank You