PF1010 HAM 2425 Tutorial 2 Slides PDF
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Summary
This document provides a tutorial on calculating the mass of oxygen in a given volume of air. It uses the ideal gas law and mole fraction, and shows a solved example, with calculations and steps.
Full Transcript
Tutorial If the mole fraction of oxygen (O2) in air is 0.22, what is the mass of oxygen in 1.0 L of air at 20 °C and 1.0 atm (atmosphere) pressure, assuming ideal behaviour? Use R = 0.082 L atm mol−1 K−1 Need PV = nRT, but solving for n Need to convert °C to K Need Molecular Mass of...
Tutorial If the mole fraction of oxygen (O2) in air is 0.22, what is the mass of oxygen in 1.0 L of air at 20 °C and 1.0 atm (atmosphere) pressure, assuming ideal behaviour? Use R = 0.082 L atm mol−1 K−1 Need PV = nRT, but solving for n Need to convert °C to K Need Molecular Mass of O2 (32 g mol−1 ) Tutorial solution 𝑃𝑉 20 °C = 273.15 + 20 PV = nRT, but solving for n so 𝑛= = 293.15 K 𝑅𝑇 (1.0 atm)(1.0 L) (1.0 L atm) n= = (293.15 K)(0.082 L atm mol−1 K−1) (24.038 L atm mol−1) n = 0.042 mol x(O2) = 0.22, so n(O2) = 0.22 x 0.042 mol = 0.00924 mol Mass O2 (in 1 L) = 32 g mol−1 x 0.00924 = 0.296 g
