CHM 1311 Lecture Notes - Lecture 10: Calcium Bicarbonate, Chemical Equilibrium, Reaction Quotient
6 Oct 2016
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Chm1311 d professor wendy pell: equilibrium (ch 14) Dynamic equilibrium (reversible reactions) i. e 2no2 -> n2o4 but then n2o4 -> 2no2 thus 2n02 n2o4. Rate of production = rate of decomposition; individual molecules continuously combine and decompose. The concentration changes as reactions occur; equilibrium of concentration is reached when substantial amount of both gases are present; ratio of concentration of reactants and products have reached a constant value. Dynamic equilibrium only occurs in a closed system. Time to reach equilibrium depends on the chemicals reacting: i. e caco3 + co2 + h2o ca(hco3)2 keq = 2. 6 x 10-5. Equilibrium constant kp rate of production kd rate of decomposition (reactants) i. e 2n02 n2o4 kp = [no2]2 kd = [n2o4] Law of mass action if reversible reaction is in equilibrium at a given temperature, then the ratio of concentrations of products to concentrations of reactants, each raised to the power of their stoichiometric coefficients is a constant (k)
