The Nature of Gases
Observing Gases Pressure
Gas pressure is the name given to the force exerted by gas particles colliding with the wall of their container.
Alternative Unit of Pressure
approximately:
1 atm = bar1
atm = 760 torr 1
torr = 1 mm Hg
1 atm = 101324.99766353 pa
The Ideal Gas Laws
The Experimental Observations Applications of the Ideal Gas Law
Molar Volume and Gas Density
Density of a gas at STP. The formula D= M/V is used at STP with M being equal to the molar mass and V being molar volume of a gas
Gase; in Mixtures and Reaction
Mixtures of Gases
The Stoichiometry of Reacting Gases
Molocular Motion
Diffusion and Effusion
- diffusion and effusion of gases Diffusion occurs when gas molecules disperse throughout a container.
- Effusion occurs when a gas passes through an opening that is smaller than the mean free path of the particles, that is, the average distance traveled between collisions. Effectively, this means that only one particle passes through at a time.
The Kinetic Model of Gases
The kinetic theory of gases is a scientific theory that explains the microscopic properties of gases, for example, temperature and volume, taking into account the molecular structure and microscopic compositions of gases. The theory states that the pressure of gases does not result from static repulsion between the molecules, but from dynamic collisions between the molecules, which have speed and momentum.
The Maxwell Distribution of Speeds
The Distribution of Molecular Speeds?
Real Gases
Deviations from Ideality Equations of State of Real Gases C E, The Liquefaction of Gases
Intermolecular Forces
The Origin of Interm olecular Forces
- Ion-Dipole Forces
- Dipole-Dipole Forces
- London Forces
- Hydrogen Bonding
- Repulsions