Part 1: One assumption we make in Kinetic Molecular Theory is that gas particles have no volume (but still have mass) and the volume of the gas is the volume of the container the gas occupies.

a.) Using 1 L of nitrogen at room temperature (25°C) at 1atm of pressure, how many moles of nitrogen is this?

b.) How many molecules is this? How many atoms is this?

c.) The radius of a nitrogen atom is 75pm. What is the volume of a nitrogen atom, assuming atoms are spherical?

d.) What is the total volume of nitrogen atoms in 1 L of nitrogen under these conditions?

e.) What percent of the volume is occupied by the gas molecules?

f.) How far apart are these gas molecules?

g.) What is in the space between the gas particles?

Part 2: Gases can be assumed to be ideal at sufficiently high temperature and sufficiently low pressures. Using this principle, what is the pressure of nitrogen from number 2 when the percent of the volume occupied by the gas molecules is 1%?