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18 Nov 2019
Balance the following two oxidation-reduction reactions in acid solutions. a) 1. MnO^-_4(aq) + Br^- (aq) rightarrow Mn^2+(aq) + Br_2(l) b) VO^+_2 + Zn rightarrow VO^2+ + n^2+ Given the following reaction and half-cell potentials below: 2 Al(s) + 3 Mg^2+(aq) rightarrow 2 Al^3+(aq) + 3 Mg(s) Al^3+(aq) +3e^- rightarrow Al(s) E degree = -1.66 V Mg^2+(aq) + 2 e^- rightarrow Mg(s) E degree = -2.37 V a) Identify which species is being oxidized and which is being reduced. b) CALCULATE the cell potential under standard conditions (E degree). c) Use the half-cell potentials above to calculate Delta G degree for the reaction.
Balance the following two oxidation-reduction reactions in acid solutions. a) 1. MnO^-_4(aq) + Br^- (aq) rightarrow Mn^2+(aq) + Br_2(l) b) VO^+_2 + Zn rightarrow VO^2+ + n^2+ Given the following reaction and half-cell potentials below: 2 Al(s) + 3 Mg^2+(aq) rightarrow 2 Al^3+(aq) + 3 Mg(s) Al^3+(aq) +3e^- rightarrow Al(s) E degree = -1.66 V Mg^2+(aq) + 2 e^- rightarrow Mg(s) E degree = -2.37 V a) Identify which species is being oxidized and which is being reduced. b) CALCULATE the cell potential under standard conditions (E degree). c) Use the half-cell potentials above to calculate Delta G degree for the reaction.
Elin HesselLv2
14 Mar 2019