The Apparent Molecular Weight of Air Experiment 1: Study the Relationship Between Volume and Temperature for a Sample of Air Lab Results Record the data you collected for volume and temperature in the table below. Volume of Air in the Syringe (mL) Total Volume of Air (mL) Temperature (ºC) 75 225.0 21.5 58.6 208.6 0 89.1 239.1 40 104.4 254.4 60 119.7 269.7 80 135.0 285.0 Create and a graph of total volume of air (y-axis) versus the temperature (x-axis). What is the relationship between volume and temperature? The volume increases as the temperature increases. Experiment 2: Study the Relationship Between Volume and Pressure for a Sample of Air Lab Results Record the data you collected for volume and temperature in the table below. Volume of Air (mL) Pressure (atm) 1/Pressure (atm–1) Data Analysis Create and save a graph of total 1/pressure (y-axis) versus volume of air (x-axis).
Experiment 3: Measure the Mass of Air Lab Results Record the data you collected for mass and pressure in the table below. Mass of Flask and Air (g) Pressure (atm) Data Analysis Calculate and record the following data in the table below. To calculate the number of moles and molar mass use the equations derived from the ideal gas law. Mass of Air (g) Number of Moles of Air Molar Mass of Air (g/mol)
Conclusions The molar masses discussed here are for dry air, but air often has some water vapor mixed in with it. Would you expect the apparent molar mass of wet air to be less or more than of dry air? Explain. Below is a graph of the mass of air as a function of the pressure. How does the data appear to be related? The relattion is consitenet when the mass increse the prusser increse.