CHE 2B Lecture Notes - Lecture 7: Chemical Equilibrium, Haber Process, Zinc Chloride
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CHE 2B Full Course Notes
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Chemical equilibrium: reactants products, at equilibrium there is a balance between reactants converting into products and products converting into reactants. Outline: definition and examples of chemical equilibrium, equilibrium constants, gas phase equilibrium, chemical activity, heterogeneous equilibrium, calculations using the equilibrium constant, equilibrium problems, le chatelier principles. Hgcl2(s) > hg2+(aq) + 2cl-(aq: equilibrium of chemical reactions, condensation of ammonia haber process . Equilibrium constant: consider a generic reaction aa + bb cc +dd, the equilibrium constant is defined as: [] indicates concentrations: large kc indicates that equilibrium is shifted toward the products. The meaning of equilibrium constants: kc > 0 always! If kc >> 1 then equilibrium is strongly shifted to the product side. If kc ~ reactants and products are balanced at equilibrium. If kc ~0 then equilibrium is strongly shifted to the reactants side: example, hydrogen gas reacts with iodine gas to form hydrogen iodide hi(g) at. T=750 c. find kc from the equilibrium gas concentrations:
