Balance the following reaction using the lowest integer coefficients

1)Balance the following reaction using the lowest integer coefficients.Br2(aq) + Ti2+(aq) → Ti3+(aq) + Br−(aq)2) Balance the following half reactions using the lowest possible whole number coefficients, in acidic conditions.(Enter coefficients for one and zero- blanks will be marked incorrect.)Bi(s) + H+(aq) + H2O(l) + e− ⇌ BiO+(aq) + H+(aq) + H2O(l) + e−ClO4−(aq) + H+(aq) + H2O(l) + e− ⇌ ClO3−(aq) + H+(aq) + H2O(l) + e−3) Balance the following reaction using the lowest possible whole number coefficients, in acidic conditions.(Enter coefficients for one and zero- blanks will be marked incorrect.)Mn2O3(s) + FeOH+(aq) + H+(aq) + H2O(l) + OH−(aq) → Mn2+(aq) + Fe2O3(s) + H+(aq) + H2O(l) + OH−(aq)4) Balance the following half reactions using the lowest possible whole number coefficients, in basic conditions.(Enter coefficients for one and zero- blanks will be marked incorrect.)I−(aq) + H2O(l) + OH−(aq) + e− ⇌ IO−(aq) + H2O(l) + OH−(l) + e−Hg2O(aq) + H2O(l) + OH−(aq) + e− ⇌ Hg(l) + H2O(l) + OH−(aq) + e−5) Balance the following reaction using the lowest possible whole number coefficients, in basic conditions.(Enter coefficients for one and zero- blanks will be marked incorrect.)ClO3−(aq) + Cu(s) + H2O(l) + OH−(aq) + H+(aq) → Cl−(aq) + Cu2O(s) + H2O(l) + OH−(aq) + H+06)Determine Ecell for the following unbalanced redox reaction, in the direction shown. Use the half reactions and potentials provided.Report your answer to three decimal places in standard notation (i.e. 1.234 V).Reaction E° (V)Elemental RedoxAu3+(aq) + 3e− ⇌ Au(s) 1.498Al3+(aq) + 3e− ⇌ Al(s) -1.662Acidic RedoxMnO2(s) + 4H+(aq) + 2e− ⇌ Mn2+(aq) + 2H2O(l) 1.224H3AsO4(aq) + 2H+(aq) + 2e− ⇌ HAsO2(aq) + 2H2O(l) 0.560Basic RedoxCrO42−(aq) + 4H2O(l) + 3e− ⇌ Cr(OH)3(s) + 5OH−(aq) -0.130AsO43−(aq) + 2H2O(l) + 2e− ⇌ AsO2−(aq) + 4OH−(aq) -0.710A) Mn2+(aq) + CrO42−(aq) → MnO2(s) + Cr(OH)3(s) (Acid-Base)B) MnO2(s) + Au(s) → Mn2+(aq) + Au3+(aq) (Acid-Elemental)C) CrO42−(aq) + Au(s) → Cr(OH)3(s) + Au3+(aq) (Base-Elemental)D) CrO42−(aq) + AsO2−(aq) → Cr(OH)3(s) + AsO43−(aq) (Base-Base)7) Use the reduction potentials, the unbalanced half reactions and the unbalanced chemical equation below to answer the following questions:Reaction E° (V)Cu2+(aq) + 2e− ⇌ Cu(s) 0.342K+(aq) + e− ⇌ K(s) -2.931Cu(s) + K+(aq) → Cu2+(aq) + K(s)A. Determine Ecell (in V) for this reaction in the direction shown. Report your answer to three decimal places in standard notation (i.e. 1.234 V).B.Determine ΔG° (in kJ) for this reaction. Report your answer to three significant figures in scientific notation (i.e. 1.23e4 kJ).8 ) 1. Determine Ecell (in V) for a cell composed of a Cu electrode in a solution of Cu+ coupled to a standard hydrogen electrode (SHE) under standard conditions. Report your answer to three decimal places in standard notation (i.e. 1.234 V).Cu+(aq) + e− ⇌ Cu(s) E° = 0.521 V9)Determine Ecell (in V) at 298.15 K for a cell composed of a Cu electrode in a solution of 0.627 M Cu+ coupled to a platinum electrode in a solution where the [H+] is 0.781 M and the partial pressure of H2 is 0.466 atm. Report your answer to three decimal places in standard notation (i.e. 1.234 V).10) Use the reduction potentials and the unbalanced chemical equation below to answer the following questions:Pb2+ (aq) + Cs (s) → Pb (s) + Cs+ (aq)Half-cell reaction E° (V)Pb2+(aq) + 2e− ⇌ Pb(s) -0.126Cs+(aq) + e− ⇌ Cs(s) -3.026A. Determine Ecell (in V). Report your answer to three decimal places in standard notation (i.e. 1.234 V)B.Determine ΔG° (in kJ/mol). Report your answer to three significant figures in scientific notation (i.e. 1.23e4 kJ).11) Determine ΔE (in V) for an electrochemical cell at 31.04 °C composed of a Sn electrode in a solution of 0.0271 M Sn2+ coupled to a Sn electrode in a solution of 1.125 M Sn2+ . Report your answer to three decimal places in standard notation (i.e. 1.234 V).Sn2+(aq) + 2e− ⇌ Sn(s) E° = -0.138 V

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