• Shuffle
Toggle On
Toggle Off
• Alphabetize
Toggle On
Toggle Off
• Front First
Toggle On
Toggle Off
• Both Sides
Toggle On
Toggle Off
Toggle On
Toggle Off
Front

### How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key

Play button

Play button

Progress

1/9

Click to flip

### 9 Cards in this Set

• Front
• Back
 Kinetic Molecular Theory 1.Gas molecules are dimensionless points 2.temperature is an indirect measure of molecular kinetic energy (higher temp = faster rxn) 3. Gas mlcls are in canstant, random, straighty- line motion 4. Gas mlcls collide w/ each other and the container walls with no loss of energy 5. Gas mlcls exert no attractice/ repulsive force on on another Pressure ration of force exerted divided by the surface area over which the force is done - force is caused by collisions - barometer and manometer * Pv= nRT Combined Gas Law Equation * P1V1/n1T1 = P2V2/n2T2 -Rigid container- neither expands or contracts, initial and final volumes equal -Closed System- nothing in, nothing out, initial and final moles equal -Insothermal- constant temp. -cancel out variables that don't change in the problems Boyle's Law -if you study the P and V of a gas, you get Boyle's Law: * P1V1= P2V2 (smaller volume= higher pressure) Charles' Law -Shows relationship between V and T of a gas -provides basis for concept of absolute zero (0= 0 volume) * V1/T1 = V2/T2 Avogadro's Principle -When you study the volume and moles of a gas * V1/n1 = V2/n2 Dalton's Law of Partial Pressures -if you have a mixture of gases, then the total pressure is simply equal to the sum of each of the individual partial pressures * Ptot= Pn -add the gase pressures together if they are simply combined in a container Molecular Speed -gas mlcls are in constant motion, but do not travel at one constant speed -temp and molar mass effect speed -Boltzmann Distribution- at higher temps. the curve flattens out more and stretches *Urms = square root of 3RT/M Effusion and Diffusion -Effusion- escape of a gas through a small hole -Diffusion- spreading of one gas through another * U1/U2 =square root of m2/m1 -to compare rates of diffusion or effusion