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Physics Chapter 14

QuestionAnswer
Many gases follow these three laws... Boyle's Law, Charles's Law, and Guy-Lussac's Law
Boyle's Law Temperature is being held constant. The volume varies inversely with the amount of pressure being exerted on it. PV = constant or P = constant/V
Charles's Law Pressure is being held constant. The constant pressure is directly proportional to the absolute temperature. V/T = constant or V = constant * T
Guy-Lussac's Law The pressure exerted by a gas held at constant volume is proportional to the absolute temperature. P/T = constant or P = constant * T
What's held constant in each rule? Boyle's Law = constant T Charles's Law = constant P Guy-Lussac's Law = constant V
Tip about Temperature Temp units always need to be in kelvin because converting between units is addition wile pressure and volume are multiplication. Things just won't stay the same.
Tip about R R is the universal gas constant. It varies depending on the unit (both of which are in the formula sheet).
A helpful equation to use for when you're comparing things... P1V1/P2V2 = T1/T2 or P1V1/T1 = P2V2/T2
Avogadro's Number Na = 6.02*10^23 molecules
Formulas for mole n = m/M (mole = mass divided by molar mass) n = N/Na (mole = total number of molecules / Avagadro's number)
kB (Boltman's constant) Equals R/Na, so it can be inserted into the ideal gas law equation like -> PV=NKbT
First Postulate of Kinetic Theory of Gases A gas consists of a large number of molecules moving in random directions with a variety of speeds.
Second Postulate of Kinetic Theory of Gases The average distance between any molecule in a gas is large compared to the size of an individual molecule (PE is considered neglible, only KE matters).
Third Postulate of Kinetic Theory of Gases The molecules obey the laws of classical mechanics and are presumed to interact with each other only when they collide.
Fourth Postulate of Kinetic Theory of Gases Collisions between molecules or between a molecule and the side walls of the container are perfectly elastic (energy will be conserved).
Average Kinetic energy Per Molecule Equations KE = 1/2mvrms^2 (average KE depends on the average of the squares of speed) KE = 3/2kbT
Internal Energy Exists in all objects, whether solid, liquid or gas. Consists of the total potential and kinetic energy of all the atoms in the substance.
Main Difference Between Solids and Gases Solids have potential energy, but the molecules in gases are moving so quickly that they DON'T.
U Equation (Total Kinetic Energy) U = KE = NKE (total number of molecules times average amount of kinetic energy per molecule) U = 3/2NkT U = 3/2nRT
Grams to Moles Grams / Molar Mass
Moles to Grams Moles * Molar Mass
Moles to Molecules Moles * Avagadro's number
Molecules to Moles Molecules / Avagadro's number
Tip about fluids and pressure To find the pressure of an object submerged in water, you can use Patm + pgh
Tip about the type of forces that work on a balloon Fb goes up, mass of the air and mass of the balloon (cargo, etc), go down. Usually, if there's skin present, the volume of the hot and cold air are equivalent.
Which R do you use when? You use 0.08206 for pressure in atm and volume in L. You use 8.314 for pressure in Pa and volume in m^3.
How to find average speed of molecules of a gas quick vrms = square root of (3RT/M) R = 8.314 T = temp in Kelvin M = molar mass in kg/mol
TIP FOR IDEAL GAS LAWS MAKE SURE YOUR VALUES MATCH THE R YOU'RE USING! ALSO YOUR MASS OR MOLES SHOULD ALWAYS BE IN KG!
Tip for converting F to K You have to subtract by 32 first, then divide by 1.8!
Created by: smurtab
 

 



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