Answer Happy

ata I Calculate the number of moles of magnesium. Calculate how many moles of hydrogen you would predict to end up with Find the pressure of the dry hydrogen gas (partial pressure of H2). Find the volume of the hydrogen gas produced. Use combined gas law to convert H, gas volume to those at STP.(P.V./T, = P.V./T,) Divide volume found at STP by the number of moles to get the experimentally determined molar volume at STP.
+ Mg(s) + HCl(aq) MgCl(aq) + H (8) You will make an experimental determination of the number of moles of hydrogen molecules produced and volume occupied by these molecules. The combined gas law will be used to correct this volume of hydrogen since it is being collected under laboratory conditions instead of STP. Your corrected volume and your calculated number of moles of hydrogen will be used to calculate the molar volume of the hydrogen gas. Since the hydrogen gas is collected by downward displacement of water. Consequently, at the end of the experiment the gas in the tube will really be a mixture of hydrogen gas and water vapor. We must then subtract the water vapor pressure from the atmospheric pressure. Water vapor is easily obtained from a table since it depends only on the temperature of the water, a P.... P (barometer) (table) (for calculation) Water Vapor Pressure Table Temperature Pressure (mmHg) .0 4.6 5.0 6.5 Pressure (mmHg) 17.0 17.5 18.1 18.6 19.2 19.8 Temperature (°C) 19.5 20.0 20.5 21.0 21.5 22.0 22.5 23.0 23.5 24.0 24.5 25.0 26.0 10.0 12.5 15.0 15.5 16.0 16.5 17.0 17.5 18.0 18.5 19.9 9.2 10.9 12.8 13.2 13.6 14.1 14.5 15.0 15.5 16.0 16.5 Temperature (°C) 27.0 28.0 29.0 30.0 35.0 40.0 50.0 60.0 70.0 80.0 90.0 95.0 100.0 20.4 Pressure (mmHg) 26.7 28.3 30.0 31.8 42.2 55.3 92.5 149.4 233.7 355.1 525.8 633.9 760.0 21.1 21.7 22.4 23.1 23.8 25.2
Mass of magnesium O® 300 g initial temp of water initial Volume 22.6°C 41.5 ml Final Volume 4.1ml Final temperature 22.9°c