CHE 1302 Lecture Notes - Lecture 19: Standard Cell, Intensive And Extensive Properties, Voltmeter
Document Summary
Baker | che 1302 | summer 2017 | lecture 19 | page 1. We want to be able to compare numbers (potentials) that will tell us how much a particular material. wants to oxidize or reduce but any electrode only represents a half-reaction. It"s impossible to measure the absolute potential of an individual electrode. Provides a reference for measuring other electrode potentials: all we can measure is the combined potential for the whole cell ((cid:1867)(cid:1876)(cid:1856)(cid:1853)(cid:1872)(cid:1867)(cid:1866)+(cid:1870)(cid:1857)(cid:1856)(cid:1873)(cid:1855)(cid:1872)(cid:1867)(cid:1866)) (cid:1834)(cid:2870) (cid:4666)(cid:1859)(cid:4667) with (cid:1842)=(cid:883) (cid:1854)(cid:1853)(cid:1870) is bubbled over an inert platinum electorde into an aqueous solution with. [(cid:1834)+ (cid:4666)(cid:1853)(cid:1869)(cid:4667)]=(cid:883)(cid:1839) (cid:2779)(cid:2164)+ (cid:4666)(cid:2183)(cid:2199), (cid:2778)(cid:4667)+(cid:2779)(cid:2187) (cid:1374)(cid:2164)(cid:2779) (cid:4666)(cid:2189), (cid:2778) (cid:2183)(cid:2202)(cid:2195)(cid:4667) She is arbitrarily assigned a potential of exactly 0v: everything else is based off of this starting point. A measure of the tendency for reduction to occur at an electrode. All half-reactions are written as reductions with eo given for the reduction relative to she. Eo values are tabulated (e. g. appendix ii: use them to calculate overall eo cell.
