CHEM-C 243 Lecture Notes - Lecture 18: Line Notation, Strong Electrolyte, Faraday Constant
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Section 1- balancing oxidation-reduction equations: oxidation-reduction (redox) reactions- electron transfer reactions. Results in generation of electric current (electricity) or caused by imposing an electric current. Oxidation- loss of electron(s) by a species; increase in oxidation number; increase in oxygen. Reduction- gain of electron(s) by a species; decrease in oxidation number; increase in hydrogen: electrochemical processes- redox reactions in which: Energy released by a spontaneous reaction is converted to electricity. Electrical energy is used to cause a nonspontaneous reaction to occur: red exponents are oxidation numbers, half-reaction- overall reaction is split into two half-reactions, one involving oxidation and one reduction. Reduction- note: stays: half-reaction method for balancing redox reactions in acidic solution. Some reactions do not balance just using coefficients; electrons do not always balance by running reactions once. Write separate equations for oxidation and reduction half-reactions. For nonbasic aqueous solutions: balance by adding ; if you need 3 oxygens, add 3 waters.
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