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17 Cards in this Set

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Moles (n) =
grams/atomic weight or molecular weight

NOTE: Atomic weight aka molar mass (MM or M)
A mole is defined by
# of C atoms in 12g of 12C.
# of C atoms in 12g of 12C is
Avogadro's Number = 6.022x10>23
6.022x10>23amu =
1g
Mega, Kilo, Deci, Centi
10>6, 10>3, 10>-1, 10>-2
Milli, Micro, Nano, Pico, Femto
10>-3, 10>-6, 10>-9, 10>-12, 10>-15
Percent Yield =
(Actual Yield/Theoretical Yield)x100
Plank's Quantum Theory
delta E = hf
h, Plank's Constant
6.6x10>-34 j s
Ideal Gas Law
PV = nRT
R, Universal Gas Constant
0.08206 L atm K>-1 mol>-1

or

8.314 j K>-1 mol>-1
Partial Pressure
Pa=Xa(Ptot)

total pressures of gaseous mixture times the mole fraction of the particular gas
Planck's quantum theory states
father of quantum mechanics. demonstrates that electromagnetic energy is quantized (comes only in discrete units related to the wave frequency). if we transfer energy from one point to another via an electromagnetic wave, and we wish to invrease the amount of energy that we are transferring without changing the frequency. we can only change the energy in discrete increments given by the equation
Dalton's Law
Ptot=P1+P2+P3...
Dalton's Law States
tot pressure exerted by a gaseous mixture is the sum of the partial pressures of each of its gases.
Derived from the ideal gas law and Dalton's law --> average translational kinetic energy and the temperature of a gas
K.E.avg = 3/2 RT
Graham's Law
V1/V2 = sqRt (m2) / sqRt (m1)