{"id":2118,"date":"2017-05-10T07:44:53","date_gmt":"2017-05-10T07:44:53","guid":{"rendered":"http:\/\/www.experimentoscientificos.es\/?p=2118"},"modified":"2017-05-10T07:54:30","modified_gmt":"2017-05-10T07:54:30","slug":"potencial-de-oxidacion","status":"publish","type":"page","link":"https:\/\/www.experimentoscientificos.es\/en\/potencial-de-oxidacion\/","title":{"rendered":"Oxidation Potential"},"content":{"rendered":"

The standard reduction potential (or negative oxidation potential) is the tendency of a chemical compound or element to reduce (or oxidise).<\/p>\n

For an oxidation-reduction reaction to occur, because it is an electron transfer, there must be an element that gives up electrons (oxidises) and another element that accepts electrons (reduces).<\/p>\n

In order to be able to know which reaction is likely to produce an oxidation or a reduction, the potential difference of the components is looked at, and in this way it is known which one will be reduced and which one will be oxidised.<\/p>\n

The reference value is given by Hydrogen, which is taken as the 0-value reference.<\/p>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
Reduction Half-Reaction Eo<\/sup>, V<\/td>\n<\/tr>\n
Acidic Solution<\/td>\n<\/tr>\n
F2<\/sub>(g) + 2e–<\/sup> \u2192 2 F–<\/sup>(aq)<\/td>\n+2.866<\/td>\n<\/tr>\n
O3<\/sub>(g) + 2H+<\/sup>(aq) + 2e– <\/sup>\u2192 O2<\/sub>(g) + H2<\/sub>O(l)<\/td>\n+2.075<\/td>\n<\/tr>\n
S2<\/sub>O8<\/sub>2<\/sup>–<\/sup>(aq) + 2e–<\/sup> \u2192 2SO4<\/sub>2<\/sup>–<\/sup>(aq)<\/td>\n+2.01<\/td>\n<\/tr>\n
H2<\/sub>O2<\/sub>(aq) + 2H+<\/sup>(aq) +2e–<\/sup> \u2192 2H2<\/sub>O(l)<\/td>\n+1.763<\/td>\n<\/tr>\n
MnO4<\/sub>–<\/sup>(aq) + 8H+<\/sup>(aq) + 5e–<\/sup> \u2192 Mn2<\/sup>+<\/sup>(aq) + 4H2<\/sub>O(l)<\/td>\n+1.51<\/td>\n<\/tr>\n
PbO2<\/sub>(s) + 4H+<\/sup>(aq) + 2e–<\/sup> \u2192 Pb2<\/sup>+<\/sup>(aq) + 4H2<\/sub>O(l)<\/td>\n+1.455<\/td>\n<\/tr>\n
Cl2<\/sub>(g) + 2e–<\/sup> \u2192 2Cl–<\/sup>(aq)<\/td>\n+1.358<\/td>\n<\/tr>\n
Cr2<\/sub>O7<\/sub>2<\/sup>–<\/sup>(aq) + 14H+<\/sup>(aq) + 6e–<\/sup> \u2192 2Cr3<\/sup>+<\/sup>(aq) + 7H2<\/sub>O(l)<\/td>\n+1.33<\/td>\n<\/tr>\n
MnO2<\/sub>(s) + 4H+<\/sup>(aq) +2e–<\/sup> -> Mn2<\/sup>+<\/sup>(aq) + 2H2<\/sub>O(l)<\/td>\n+1.23<\/td>\n<\/tr>\n
O2<\/sub>(g) + 4H+<\/sup>(aq) + 4e–<\/sup> \u2192 2H2<\/sub>O(l)<\/td>\n+1.229<\/td>\n<\/tr>\n
2IO3<\/sub>–<\/sup>(aq) + 12H+<\/sup>(aq) + 10e–<\/sup> \u2192 I2<\/sub>(s) + 6H2<\/sub>O(l)<\/td>\n+1.20<\/td>\n<\/tr>\n
Br2<\/sub>(l) + 2e–<\/sup> \u2192 2Br–<\/sup>(aq)<\/td>\n+1.065<\/td>\n<\/tr>\n
NO3<\/sub>–<\/sup>(aq) + 4H+<\/sup>(aq) + 3e–<\/sup> \u2192 NO(g) + 2 H2<\/sub>O(l)<\/td>\n+0.956<\/td>\n<\/tr>\n
Ag+<\/sup>(aq) + e–<\/sup> \u2192 Ag(s)<\/td>\n+0.800<\/td>\n<\/tr>\n
Faith3<\/sup>+<\/sup>(aq) + e–<\/sup> \u2192 Fe2<\/sup>+<\/sup>(aq)<\/td>\n+0.771<\/td>\n<\/tr>\n
O2<\/sub>(g) + 2H+<\/sup>(ag) + 2e–<\/sup> \u2192 H2<\/sub>O2<\/sub>(aq)<\/td>\n+0.695<\/td>\n<\/tr>\n
I2<\/sub>(s) + 2e–<\/sup> \u2192 2I–<\/sup>(aq)<\/td>\n+0.535<\/td>\n<\/tr>\n
Cu2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Cu(s)<\/td>\n+0.340<\/td>\n<\/tr>\n
SO4<\/sub>2<\/sup>–<\/sup>(aq) + 4H+<\/sup>(aq) + 2e–<\/sup> \u2192 2H2<\/sub>O(l) + SO2<\/sub>(g)<\/td>\n+0.17<\/td>\n<\/tr>\n
Sn4<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Sn2<\/sup>+<\/sup>(aq)<\/td>\n+0.154<\/td>\n<\/tr>\n
S(s) + 2H+<\/sup>(aq) + 2e–<\/sup> \u2192 H2<\/sub>S(g)<\/td>\n+0.14<\/td>\n<\/tr>\n
2H+<\/sup>(aq) + 2e–<\/sup> <\/span>\u2192 H2<\/sub>(g)<\/span><\/td>\n0<\/span><\/td>\n<\/tr>\n
Pb2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Pb<\/td>\n-0.125<\/td>\n<\/tr>\n
Sn2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Sn(s)<\/td>\n-0.137<\/td>\n<\/tr>\n
Faith2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Fe(s)<\/td>\n-0.440<\/td>\n<\/tr>\n
Zn2<\/sup>+<\/sup> + 2e–<\/sup> \u2192 Zn(s)<\/td>\n-0.763<\/td>\n<\/tr>\n
Al3<\/sup>+<\/sup>(aq) + 3e–<\/sup> \u2192 Al(s)<\/td>\n-1.676<\/td>\n<\/tr>\n
Mg2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Mg(s)<\/td>\n-2.356<\/td>\n<\/tr>\n
Na+<\/sup>(aq) + e–<\/sup> \u2192 Na(s)<\/td>\n-2.713<\/td>\n<\/tr>\n
Ca2<\/sup>+<\/sup>(aq) + 2e–<\/sup> \u2192 Ca(s)<\/td>\n-2.84<\/td>\n<\/tr>\n
K+<\/sup>(aq) + + + e–<\/sup> \u2192 K(s)<\/td>\n-2.924<\/td>\n<\/tr>\n
Li+<\/sup>(aq) + e–<\/sup> \u2192 Li(s)<\/td>\n-3.040<\/td>\n<\/tr>\n
\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
Basic Solution<\/td>\n\u00a0<\/td>\n<\/tr>\n
O3<\/sub>(aq) + H2<\/sub>O(l) + 2e–<\/sup> \u2192 O2<\/sub>(g) + 2OH–<\/sup>(aq)<\/td>\n+1.246<\/td>\n<\/tr>\n
OCl–<\/sup>(aq) + H2<\/sub>O(l) + 2e–<\/sup> \u2192 Cl–<\/sup>(aq) + 2OH–<\/sup>(aq)<\/td>\n+0.890<\/td>\n<\/tr>\n
O2<\/sub>(g) + 2H2<\/sub>O(l) +4e–<\/sup> \u2192 4OH–<\/sup>(aq)<\/td>\n+0.401<\/td>\n<\/tr>\n
2H2<\/sub>O(l) + + 2e–<\/sup> \u2192 H2<\/sub>(aq) + 2OH–<\/sup>(aq)<\/td>\n-0.0828<\/td>\n<\/tr>\n<\/tbody>\n<\/table>","protected":false},"excerpt":{"rendered":"

The standard reduction potential (or negative oxidation potential) is the tendency of a chemical compound or element to reduce (or oxidise). For an oxidation-reduction reaction to occur, since it is a transfer of electrons, there must be an element that gives up electrons (oxidises) and another element [...].<\/p>","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"open","ping_status":"open","template":"","meta":{"_acf_changed":false,"footnotes":""},"acf":[],"yoast_head":"\nPotencial de Oxidaci\u00f3n<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.experimentoscientificos.es\/en\/potencial-de-oxidacion\/\" \/>\n<meta property=\"og:locale\" content=\"en_GB\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Potencial de Oxidaci\u00f3n\" \/>\n<meta property=\"og:description\" content=\"El potencial standard de reducci\u00f3n (o en su valor negativo de oxidaci\u00f3n) es la tendencia que tiene un compuesto o elemento 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