CHMB16H3 Lecture Notes - Lecture 9: Standard Electrode Potential, Electrochemical Cell, Oxidation State
Document Summary
Oxidation and reduction reaction (redox reactions: oxidation/reduction reactions involve the transfer of electrons and a change in oxidation state, a reducing age (reductant) is an electron donor, an oxidizing agent (oxidant) is an electron acceptor. +2 +7 +3 +2 9 balancing redox reactions step 5. Balance the oxygen atoms for each half-reaction by adding h2o step 6. Balance the hydrogen atoms foe each half-reaction *now both half-reactions should be balanced! +2 +7 +3 +2 10 balancing redox reactions step 7. Multiply and add each half reaction together to get the net equation +2 +7 +3 +2 balanced! o. Irreversible: reversing the direction of electron flow causes different half reactions to occur at one or both electrodes. Redox reactions in an electrochemical cell: ecell can be measured using a voltmeter connected between the 2 electrodes of the cell. Standard hydrogen reference electrode the 2 hald reactions are: the standard potential of this electrode is set at 0. 000v by convention.
