Using the kinetic theory of gases, calculate the following at 25C and 1 bar. Assume ideal gas behavior. a. Average kinetic energy of a helium atom. (3 points) b. Average kinetic energy of an oxygen molecule. Compare the result with what you obtained in (a) and comment on the parameters that affect the kinetic energy of an ideal gas. (5 points) c. Root mean square velocity, urms, of a helium atom. (3 points) d. Root mean square velocity, Urms, of an oxygen molecule. Compare the result with what you obtained in (c). Which gas moves faster, helium or oxygen? Explain how the mass of an atom/molecule affects its root mean square velocity. (5 points) e. Mean free path of helium gas. (3 points) f. Mean free path of oxygen gas. Compare the result with what you obtained in (e). Which gas travels further, helium or oxygen? Explain why. (5 points) Boltzmann constant: 1.38x10-23 J/K Molar mass of helium atom: 4 g/mol Molecular diameter of helium: 0.22 nm Molar mass of oxygen atom: 16 g/mol Molecular diameter of oxygen: 0.31 nm Avogadro number: 6.02x1023 number of atoms or molecules/mol