10 terms

AP Chem Final Exam Unit 2

Ideal Gas law
PV=nRT (changes in any of the variables can be tracked using : (PV=nRT [final]/ PV=nRT [initial])
Boyle's Law
Inverse relationship between pressure and volume
Charles's Law
Direct relationship between volume and temperature
Avogadro's Law
Direct relationship between volume and moles
1 atm and 273K
Standard Temperature and Pressure (STP)
Dalton's law of partial pressure
The total pressure is equal to the sum of all the individual pressures (P total = P₁ + P₂ + P₃ ...)
1. Gases are made up of small microscopic particles. 2. Particles are in constant motion and the collision with the container wall is the cause for the pressure exerted (elastic). 3. Particles are assumed to exert no force on each other (neither attract nor repel each other). 4. The average kinetic energy is assumed to be directly proportional to the Kelvin temperature of the gas.
The kinetic Molecular Theory of a Gas states that an ideal gas has the following properties:
The passage of a gas through a tiny hole into an evacuated chamber (like a perfume).
Rate of effusion
Formula is: rate of effusion for gas 1/rate of effusion for gas 2 = √M₂/√M₁. (Note: a lighter, smaller, less polar gas effuses quicker than a heavier gas).
The opposite of effusion. Example is a smell that smells throughout the room, people in front row smell it first and then it moves further back and the rows further back start to smell it.