Pre-Laboratory Assignment Name: Section: Molar Volume of Hydrogen Reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen gas. The gas was collected by water displacement at 22 C. The barometric pressure in the lab was 746 mm Hg. COPE Date: 1. The vapor pressure of water at 22 C is 19.8 mm Hg. Use Dalton's law to calculate the partial pressure of hydro- gen gas in the gas-collecting tube. 7262mm Hg x310mlx 273K 760 mmHq X295 K 10 746 mmHg=198mm Hgt PH PH = 746 mm Hg - 19.8mm Hg/ PH = 724 2 mm H 2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP. Hint: Watch your units for temperature and pressure! -= 27.41m 27.41ml 3. What is the theoretical number of moles of hydrogen that can be produced from 0.028 g of Mg? Hint: Refer to Equation 1 for the balanced equation for the reaction. 4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to calculate the molar volume (in L/mole) of hydrogen at STP

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Sure lets go through these steps one by one 1 Daltons Law states that the total pressure in a mixture of gases equals the sum of the partial pressures ... View the full answer