Ideal Gas law
PV = nRT
n = number of moles
R = universal gas constant = 8.3145 J/mol K
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Combined Gas law
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Boyle's law
P1V1 = P2V2
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Charles law
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Gay-Lussac law
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Diffusion: Rate at which two gases mix
Graham's law of diffusion
The rate of diffusion of a gas is inversely proportional
to the square root of their density or
the molar mass of the gas.
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Effusion: Rate at which a gas escapes thru pin hole
Graham's law of effusion
The rate of effusion of a gas is inversely proportional to
the square root of either the density or
the molar mass of the gas.
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Solution: Solution is a homogeneous mixture of two or more
substances.
Solute is a substance that is dissolved in the solution.
Solvent is the substance that dissolves the solute.
Solvent is present in greater amount.
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Concentration is the ratio of solute and solvent.
Concentration can be measured using molarity, molality and mole fraction.
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Molarity (M) =
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moles of solute
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liters of solution
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Molality (m) =
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moles of solute
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kg of solution
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Unit of Molarity (M) : mol/L : moles per litre
Unit of Molality (M) : mol/kg : moles per kg
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Mole fraction:
Mole fraction of a component in solution is
the number of moles of that component divided by the
total number of moles of all components in the solution.
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Mole-fraction (Xa)=
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molesa
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molesa + molesb ....
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Dilution:
Siluting a solution means adding more solvent in solution
without the addition of more solute.
MiVi = MfVf
Mi: Molarity of solution before diluting.
Vi: Volume of solution before diluting.
Mf: Molarity of solution after diluting.
Vf: Volume of solution after diluting.
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Mole: Mole is the amount of substance that contains
same number of particles as there are atoms in
Carbon-12.
One mole of substance is Avogadro's number (i.e. 6.023 x 1023).
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One mole of gas has volume of 22.4 liter at STP.
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Relation between moles and grams
1 mole = molecular weight of substance in grams.
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