CHE 1302 Lecture Notes - Lecture 14: Dynamic Equilibrium, Endothermic Process, Partial Pressure
Document Summary
Dynamic equilibrium: we are used to reactants > products. Don"t occur completely: could start from pure reactants, pure products, or mixture of r & p. Will always get to some intermediate point: equilibrium, reaction appears to stop because: @ molecular level still going: ex) of dynamic equilibrium, in each case: Concentrations, pressures, etc stay constant: equilibrium constant (k) Tells extent of equilibrium reaction (how far it goes) Gives idea of relative amounts of reactants & products: ex, starting point does not matter. Once equilibrium is reached, k ration remains constant: k ratio: Must use equilibrium concentrations: k has no units. Kc = when everything is expressed as concentrations: concentration equilibrium constant, exponent of each concentration is always stoichiometric coef cient. Always products over reactants: size of k tells what equilibrium will look like when we get there. Does not tell how quickly equilibrium is reached: if k is very large (k >> 1)
