A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen gas. The gas was collected by the water displacement in a 22 C water bath. The barometric pressure inthe lab that day was 746 mm Hg.
1. Use Dalton's law and the vapor pressure of water at 22 C to calculate the partial pressure of hydrogen gas in the gas collected tube.
2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP.
3. What is the theoretical number of moles of hydrogen gas that can be produced from 0.028 g of Mg?
4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to calculate the molar volume (in L/mol) of hydrogen at STP.
1. Use Dalton's law and the vapor pressure of water at 22 C to calculate the partial pressure of hydrogen gas in the gas collected tube.
2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP.
3. What is the theoretical number of moles of hydrogen gas that can be produced from 0.028 g of Mg?
4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to calculate the molar volume (in L/mol) of hydrogen at STP.