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Chapter 6
26
Chemistry
Undergraduate 1
12/12/2013

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Term
Volume and Temperature
Definition
Proportional
Term
Pressure
Definition
Force/Surface Area
Term
Atmosphere
Definition
760 mmHg
760 Torr
1.01325 Pascals
101.325 Kilopascals
Term
Force
Definition
mass * acceleration
Term
Pascal
Definition
1kg/m*s2
SI unit of pressure
Term
Manometers
Definition
1)open manometer= pgas=patm+deltahHg
2)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
Avogadro's Law
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 volume
1)d=m/v=PM/RT
Term
Dalton's Law
Definition
Patm=P1+P2+P3...etc...etc
the 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 randomly
3)the motion of these molecules is associated with an average kinetic energy proportional to the absolute temperature of the gas
4)They continually collide with eachother and these collisons are elastic
5)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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