# Shared Flashcard Set

Definitions
Chapter 6
26
Chemistry
12/12/2013

## Additional Chemistry Flashcards

Term
 Volume and Temperature
Definition
 Proportional
Term
 Pressure
Definition
 Force/Surface Area
Term
 Atmosphere
Definition
 760 mmHg760 Torr1.01325 Pascals101.325 Kilopascals
Term
 Force
Definition
 mass * acceleration
Term
 Pascal
Definition
 1kg/m*s2SI unit of pressure
Term
 Manometers
Definition
 1)open manometer= pgas=patm+deltahHg2)closed manometer=pgas=deltah
Term
 Boyle's Law
Definition
 Pressure and Volume are inversely proportional~as pressure increases, volume decreses
Term
 Charles' Law
Definition
 Volume and Temperature are proportional~as volume increases, temperature increases
Term
Definition
 Moles and Volume are proportional~as # of moles increases, volume increases
Term
 Amonton's Law
Definition
 Pressure and Temperature are proportional~as pressure increases, temperature increases
Term
 Ideal Gas Law
Definition
 PV=nRT
Term
 Universal Gas Constant
Definition
 R 0.08206L*atm/mol*K
Term
 Combined gas law
Definition
 P1V1/n1T1=P2V2/n2T2; where n is constant
Term
 STP
Definition
 1 atm 0 degrees celcius
Term
 SATP
Definition
 1 atm 25 degrees celcius
Term
 Molar Volume
Definition
 Volume occupied by 1 mole of gas at STP; 22.4L
Term
 Calculating Density of a gas at STP
Definition
 Divide it's molar mass by it's molar volume1)d=m/v=PM/RT
Term
 Dalton's Law
Definition
 Patm=P1+P2+P3...etc...etcthe total pressure of any mixture of gasses equals the sum of all the partial pressures of the gases in the mixture
Term
 Mole fraction
Definition
 moles of a substance/total moles in mixture
Term
 Kinetic Molecular Theory
Definition
 1)gas molecules have tiny volumes compared with the collective volume they occupy (no volume is assumed)2)they move constantly and randomly3)the motion of these molecules is associated with an average kinetic energy proportional to the absolute temperature of the gas4)They continually collide with eachother and these collisons are elastic5)There are no attraction or repulsion forces acting on these molecules
Term
 Average Kinetic Energy
Definition
 KEavg=1/2m(urms)^2
Term
 Root mean squared
Definition
 urms=the square root of (3RT/Molar mass)
Term
 Graham's Law of effusion
Definition
 rsubx/rsuby=square root of (molar mass x/molar mass y)
Term
 Effusion
Definition
 Gas escapes from it's container through a tiny hole into a region of lower pressure
Term
 Diffusion
Definition
 The spread of one substance (usually a gas or liquid) through another
Term
 van der Waals equation for real gases
Definition
 (P+n^2a/V^2)(V-nb)=nRT
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