The hydrogen gas formed in a chemical reaction is collected over water at 30.0 degrees c at a total pressure of 732 mmhg what is the partial pressure of the hydrogen gas collected

when a gas is collected over water at 30.0 deg C, the H2O vapor pressure is 32 Torr Part A:What is the partial pressure of the hydrogen gas collected in this way? at a total pressure of 732 mm Hg. - 32 Torr H2O vapor = 700. Torr H2 your answer is answer is 700 mm Hg. Part B: If the total volume of gas collected is 724 mL, what mass of hydrogen gas is collected? find moles PV = nRT (700. Torr) (0.724 Litres) = n (62.36 Torr-Litres/mol-K) (303 Kelvin) n = 0.02682 moles of H2 using molar mass, find moles: (0.02682 moles of H2) (2.016 grams H2 / mol) = 0.05407 grams of H2 your answer rounded to 3 sig figs is 0.0541 grams of H2