Gases.

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Presentation transcript:

Gases

Properties of Gases Fluids Low density Expand to fill container Effuse/ Diffuse Compressible Exert pressure

Effusion- gas particles push through a tiny opening in a container Diffusion- gas particles mix freely due to kinetic molecular theory (KMT)

Pressure Force on a surface Units of pressure 1atm=760.mmHg=101.325kPa=760.torr=1.0bar=14.7psi=101325Pa You can convert from one pressure unit to another using dimensional analysis

1atm=760.mmHg=101.325kPa=760.torr=1.0bar=14.7psi=101325Pa 2.18atm =_______ psi 823.46 mmHg=______kPa 174.21kPa =_______atm

Kinetic-Molecular Theory Assumptions large number of particles very far apart relative to their size. all collisions are elastic. no loss of kinetic energy. particles in constant, rapid, random motion no IMF exist among particles average kinetic energy depends solely on temperature

Ideal vs Real Gases Ideal gases obey all assumptions of KMT Real gases imaginary Nobel gases almost always act ideally Real gases at high pressure or low temperature IMF exist Not all of the assumptions apply