Ideal Gases and The Ideal Gas Law LG: I can perform calculations involving temperature, pressure, volume, and amount using the ideal gas law

Ideal Gases Our ideas about how gases behave are based on the assumption that gases behave “ideally”, which means: – Gas particles travel in straight lines at high speeds – Collisions with other particles and the container are perfectly elastic (no loss of kinetic energy) – The volume of the gas particles is zero relative to the size of the container – Particles of a gas are not attracted to one another – Gases do not condense into liquids when cooled

Ideal Gas Law Rearrange the equation to determine the units for R

Ideal Gas Law and Molar Volume The ideal gas law can be used to verify what we know about molar volume at STP and SATP:

Sample Problem 1

Sample Problem g of a pure gas occupies 2.10 L at 123⁰C and 99.7 kPa. Determine the molar mass of the unknown gas.

Working with “Real Gases” The behaviours of a gas are relatively ideal when the volume is large, the pressure is low, and temperatures are high. As pressure increases there are more collisions which increases attraction between particles As volume decreases there are more collisions and the volume of the gas is no longer irrelevant compared to the container As temperature decreases the particles lose kinetic energy and experience more attraction, which may result in condensation

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