Mass of Mg per Meter: 12.39 g Length of Mg Ribbon: 5.15 cm Room temperature: 21.
ID: 532442 • Letter: M
Question
Mass of Mg per Meter: 12.39 g
Length of Mg Ribbon: 5.15 cm
Room temperature: 21.5 °C
Beaker Water temperature:
Before: 19.5°C
After: 22.0°C
Average Temperature: 21.0°C
Volume of gas collected: 92.1mL
Barometric pressure: 74.25cmHg
Vapor pressure: 18.659mmHg (from Handbook of Chemistry and Physics, 81st Edition, p6-10)
Density= 0.997995g/cm^2
5. Partial Pressure of Hydrogen Gas in mmHg (Use Dalton’s Low of Partial Pressures)
6. Partial Pressure of Hydrogen Gas in atmospheres
7. Estimated Temperature of the Hydrogen Gas in ºC (Average temperature of the room temperature, the water temperature before, and the water temperature after).
8. Estimated Temperature of the Hydrogen Gas in K (Average temperature of the room temperature, the water temperature before, and the water temperature after).
9. Actual Moles of Hydrogen Gas Produced (Use the ideal gas law. This value should be similar to your answer in #3, assuming that all of the magnesium ribbon reacted.)
10. Ratio of Moles of Mg to Actual Moles of Hydrogen Gas Produced.
11. Volume that the Sample of Hydrogen Gas would Occupy at STP (Use the combined gas law).
12. Molar Volume of Hydrogen Gas at STP (Use the volume from #11 & the moles of hydrogen gas from#3)
13. Using the theoretical value of 22.4 L/mole, calculate your % error.
Explanation / Answer
Hi
5. Partial pressure of hydrogen Gas in mmHg (Use Dalton’s Low of Partial Pressures)= 74.25cmHg
6. Partial Pressure of Hydrogen Gas in atmospheres= 74.25cmHg= 742.5 mm Hg= 742.5/760 atm = 0.977 atm
7. Estimated Temperature of the Hydrogen Gas in ºC (Average temperature of the room temperature, the water temperature before, and the water temperature after) = (21.5 °C + 19.5°C + 22.0°C)/3 = 21.0°C
8. Estimated Temperature of the Hydrogen Gas in K (Average temperature of the room temperature, the water temperature before, and the water temperature after).= 21.0 + 273.15 K= 294.15 K
Thank you