You analyze a sample of unknown metal using the procedure described in the lab manual. atmospheric pressure, patm in the lab is measured as 28.52 inches of mercury (in hg). you measure the water temperature to be 2 0° c, which from the tables posted on the wall tells you the vapor pressure of water ph20(g is 17.5 mm hg from the height of the water column left in the gas collection ph2, the partial pressure of h2(g), in the gas collection tube tube. you calculate ph200 to be 0.0193 atm. calculate, in atmospheres, ph2, the partial pressure of h-/8) in the gas collection tube. atm key equations ou need to calculate ph, the partial pressure of h2 (g) in the collection tube. the gas collected is a mixture of ph2 (9) and water vapor, which has vapor pressure pus, o (g). (the vapor pressure of water can be found in a table in your textbook.) the column of water remaining in the collection tube also creates a downward pressure, all of this is balanced by atmospheric pressure, patmos, as shown in equation (2): 12] ph (9) +ph,0(g) +ph, o) patmos the ph200 term in equation (2) is the pressure due to the column of water in the collection tube above the liquid level in the beaker (see the figure on the next page). in order to calculate this pressure exerted by the water column, use the equation: 13] where p is the pressure in pascals (pa) which has the units of kg/(m s); g is the constant acceleration due to gravity (9.81 m/s'); d is the density of water in kg/n'; and h is the height in meters of the liquid water above the water level in the beaker. for this experiment, assume that the density of water is 1.00 g/cm and convert this value to kg/m for use in equation (3). after determining the pressure in pascals, kg/(m s'), you will want to convert it to atm or mmhg (1.00 atm- 101.3 kpa 760 mmhg). use the ideal gas law to calculate the moles of hydrogen gas generated, where p-ph, calculated using equation (2) 14] use the concept of molar mass for the final identification of this metal. 15) molar mass grams/mole