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73 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Phase changes |
H+
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Lithium |
LI+ |
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Sodium |
Na+ |
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Potassium |
K+ |
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Rubidium |
Rb+ |
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Cesium |
Cs+ |
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Silver |
Ag+ |
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Magnesium |
Mg2+ |
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Calcium |
Ca2+ |
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Strontium |
Sr2+ |
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Barium |
Ba2+ |
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Zinc |
Zn2+ |
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Iron (II) |
Fe2+ |
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Iron (!!!) |
Fe3+ |
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Aluminum |
Al3+ |
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Ammonium |
NH4+ |
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Fluoride |
F- |
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Chloride |
Cl- |
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Bromide |
Br- |
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Iodide |
I- |
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Oxide |
O2- |
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Sulfide |
S2- |
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Nitride |
N3- |
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Phosphide |
P3- |
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Hydroxide |
OH- |
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Cyanide |
CN- |
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Nitrate |
NO3- |
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Acetate |
C2H3O2- |
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Sulfate |
SO4 2- |
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Hydrogen sulfate (bisulfate) |
HSO4- |
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Carbonate |
CO3 2- |
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Hydrogen Carbonate |
HCO3- |
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Phosphate |
PO4 3- |
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Chlorate |
ClO3- |
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Perchlorate |
ClO4- |
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1 atm |
=760 mmHg =760 torr |
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Boyle's Law |
Volume, of fixed quantity of gas at constant Temp, is inverse proportional to Pressure. (CONSTANT n + T) V=K*1/P PV=K P1V1=P2V2 |
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Charles Law |
Volume, of fixed amount of gas at constant pressure, directly proportional to absolute Temp. (CONSTANT n + P) V=K*T V/T=K V1/T1=V2/T2 |
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Avogardro's Law |
Volume, of gas at constant T and constant P is direct proportional to # moles of gas (CONSTANT T + P) V=K*n V/n=K V1/n1=V2/n2 |
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Ideal Gas Law |
PV=nRT |
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Ideal Gas defined |
hypothetical gas that obeys Kinetic Molecular Theory and Ideal Gas Law |
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STP |
I atm 0*C |
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Combined Gas Law |
# moles constant. Doesnt apply with chemical reactions P1V1/T1 = P2V2/T2 |
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Combined Gas Law #n & V constant |
P1/T1=P2/T2 |
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Combined Gas Law Constant T |
P1V1=P2V2 |
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Combined Gas Law Constant Pressure |
V1/T1=V2/T2 |
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Ideal Gas determine Density / Molar Mass of Gas |
D = P * molar / mass ---------------------- R * Temp |
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If molar mass and Pressure is constant |
T increase D decrease |
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Daltons Law of Partial Pressure |
total pressure of mix of gases equal sum of pressure that each exert alone Ptotal = P1 + P2 + P3 + ..... |
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Gramham's Law of Effusion |
rate of effusion of gas inverse to square root of its molar mass r1 = 1 / square root (fancy M) |
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lower molar mass |
balloons go down |
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higher molar mass |
balloon go up |
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Diffusion |
spread 1 substance through out another |
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mole fraction (x) |
ration of number of moles of one component to total number moles in mix Xa = mol a / total mol |
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Partial Pressure |
Pa = Xa Ptotal |
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DeltaH |
Q phase change = DeltaH phase change * # moles |
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Heat of fusion |
Change required to change sold at its melting point to a liquid at the same temp |
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Heat of fusion |
Change required to change sold at its melting point to a liquid at the same temp |
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Heat of vaporization |
Change required to change a liquid at its boiling point to a gas at the same temp |
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Heat of sublimation |
Change required to transform a solid directly into the gas phase |
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Phase change |
Converting from one physical state to another requires the molecules to gain enough kinetic energy to overcome the intermolecular forces |
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Calculate amount of heat needed when the temperature changes |
Q= C x mass c DeltaTemp |
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Calc amount of heat needed during phase change |
Q = DeltaH x moles |
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Phase change chart |
Back (Definition) |
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Phase diagram |
Back (Definition) |
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Ideal gas equation |
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Combined gas law |
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Kinetic molecular theory |
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Real gases |
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Exotermic reaction |
reaction |
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Endothermic reaction |
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Phase changes |
Back (Definition) |
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J |
J |
H |
