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Seventy six -0. seventy six -0. seventy six iBr 2 (aq) + ~ -> Br(aq) ;. (ii) Br 2 (aq) -\-2e~ -»2Br~(aq) + 1,07 1. 07 -1 x 96487 x (+0. seventy six) -1 x 96487 x (-0. seventy six) -2 x 96487 x (-0. sixteen) AG(7; = + 146. 7kJ -1 x 96487 x ( + 1. 07) -2 x 96487 x ( + 1. 07) AG^ = - 206. five kJ for this reason (i) and (ii) provide 2Fe2 + (aq) four- Br 2 (aq) -» 2Fe3 + (aq) -f 2Br~(aq) AG = AG^ -f GJ^} - + 146. 7 -h ( - 206. five) = - fifty nine. eight kJ hence the response is energetically possible and does certainly happen. it truly is attention-grabbing at this element to enquire the explanations why iron(II) ions in aqueous ideas are quantitatively predicted by means of titration utilizing potassium manganate(VII) (permanganate) while chloride ions are absent yet by way of potassium dichromate(VI) while chloride ions are current. the information for the oxidation of chloride ions to chloride by way of (a) manganate(VII) and (b) dichromate( VI) ions lower than normal stipulations are given less than: (a) 2MnO4 (aq) -f 10Cl~(aq) + I6H three O + four- 24H 2 O four- 5Cl2(g) E~(V) response + M n O four ( a q ) + 5e~ -f 8H^O -> Mn-(aq) + 12H 2 O (i) 2MnO4 (aq) + I0e~ + 16H three O* —» 2Mn 2 "^(aq) four- 24H 2 O iC! 2 (aq) + e~ - > C l ~ ( a q ) CP(aq) -»• 4Cl 2 (aq) + e" (ii) lOCl'(aq) -> 5Cl 2 (aq) four- We~ A G * = - W J*E + 1. fifty two -5 x 96487 x ( + 1. fifty two) four- 1. fifty two AG(t = - 10 x96487 x (+1. fifty two) = -1467kJ 4-1. 36 -1. 36 -1. 36 - 1 x ninety six 487 x (-1. 36) AGJ^, = — 10 x 96487 x (-1. 36) = + 1312kJ consequently (i) and (ii) supply 2MnC>4 (aq) + 10C1" (aq) + 16H three O + -> 2Mn 2 + (aq) + 24H 2 O four- 5Cl 2 (aq) 104 ACIDS AND BASES: OXIDATION AND relief lor which AG = AG(7; + AG(% = ( - 1467) + ( -f 1312) - - a hundred and fifty five kJ therefore chloride ions are oxidised to chlorine by way of manganate(VII) less than general stipulations (b) Cr 2 CH~(aq) + 6C1"(aq) + 14H3O + -> 2Cr three + (aq) four- 21H 2 O -f 3Cl 2 (aq) response AG~* = -nh'c (i) Cr 2 O= (aq) + 6e + 14H3CT -> 2Cr three '(aq) + 21H 2 O " k12|aq) + f " -> CP(aq) Cl'(aq) ->• K'Maq) + f ' (ii) 6C1 (aq) ->~3Cl 2 (aq) + 6t>" +1,33 jf} = ^6 x 96487 x ( + 1 . three three ) +1. 36 -1,36 -1. 36 -1 x ninety six 487 x ( - 1,36) AG(T*» = -6 x 96487 x (-1,36) for that reason (i) and (ii) supply 6CP(aq) 21H 2 O + 3Cl 2 (aq) for which AG - AGg -f = ( -769) = + 18 kJ ( + 787) hence below general stipulations chloride ions should not oxidised to chlorine by means of dichromate(VI) ions. even though, it is important to stress that adjustments within the focus of the dichromate(VI) and chloride ions alters their redox potentials as indicated by means of the Nernst equation. consequently, while targeted hydrochloric acid is extra to reliable potassium dichromate and the combination warmed, chlorine is liberated. Equilibrium constants from electrode potentials we've seen that the lively feasibility of a response might be deduced from redox strength facts. it's also attainable to infer the theoretical equilibrium place for a response. In bankruptcy three we observed that after AG = zero the process is at equilibrium. when you consider that AG = — nFE, which means the opportunity of the telephone has to be 0. give some thought to once more the response + Zn(s) -* Cu(s) + Zn 2 f (aq) ACIDS AND BASES: OXIDATION AND relief a hundred and five At equilibrium at 298 ok the electrode strength of the half-reaction for copper, given nearly through needs to equivalent the electrode power for the half-reaction for zinc, given nearly through therefore, Efn + ^- log 10 [Zn 2 + (aq)] = Eg, -f ^- log 10 [Cu 2+ (aq)] — z.