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17 Cards in this Set
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Moles (n) =
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grams/atomic weight or molecular weight
NOTE: Atomic weight aka molar mass (MM or M) |
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A mole is defined by
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# of C atoms in 12g of 12C.
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# of C atoms in 12g of 12C is
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Avogadro's Number = 6.022x10>23
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6.022x10>23amu =
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1g
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Mega, Kilo, Deci, Centi
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10>6, 10>3, 10>-1, 10>-2
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Milli, Micro, Nano, Pico, Femto
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10>-3, 10>-6, 10>-9, 10>-12, 10>-15
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Percent Yield =
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(Actual Yield/Theoretical Yield)x100
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Plank's Quantum Theory
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delta E = hf
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h, Plank's Constant
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6.6x10>-34 j s
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Ideal Gas Law
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PV = nRT
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R, Universal Gas Constant
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0.08206 L atm K>-1 mol>-1
or 8.314 j K>-1 mol>-1 |
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Partial Pressure
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Pa=Xa(Ptot)
total pressures of gaseous mixture times the mole fraction of the particular gas |
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Planck's quantum theory states
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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
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Dalton's Law
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Ptot=P1+P2+P3...
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Dalton's Law States
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tot pressure exerted by a gaseous mixture is the sum of the partial pressures of each of its gases.
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Derived from the ideal gas law and Dalton's law --> average translational kinetic energy and the temperature of a gas
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K.E.avg = 3/2 RT
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Graham's Law
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V1/V2 = sqRt (m2) / sqRt (m1)
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