Question

Data:

Mass of Magnesium ribbon per meter (g/m) : 0.076g/m Length of magnesium ribbon (cm):3.8 Room temp: 24.0 C Water temp before the reaction: 16.5 C Water temperature after the reaction:18.0 C Atmostpheric or barometric pressure (cmHg): 73.4cmHg Water Vapor pressure at the average temp (mmHg): 15.878 mmHg Volume of gas collected (mL): 89.2mL

1. Mass of Mg ribbon reacted ? 2.Moles of Mg ribbon reacted? 3.Theoretical moles of hydrogen gas produced (based on the limiting reactant)? 4.Atmospheric pressure in mmHg? Partial pressure of hydrogen gas in mmHg (use dalton's law of partial pressure) 6.Partial pressure of hydrogen gas in atmospheres 7.Estimated temp of the hydrogen gas in C (average temp of all three collected temp) 8. Estimated temp of the hydrogen ga in K (average temp of all three collected temp) 9. Experimental (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 the moles of the Mg ribbon to the experimental 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 and the moles of hydrogen gas from #9) 13. Using the theoretical value of the molar volume as 22.4 L/mol, calculate the percent error

Answer 1