CHM 1311 Chapter Notes - Chapter 14: Calcium Bicarbonate, Chemical Equilibrium, Equilibrium Constant

• School: University of Ottawa
• Department: Chemistry
• Course: CHM 1311
• Professor: Wendy Pell

Document Summary

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] 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)