Use the data in Appendix 2 to predict whether or not the following reactions are feasible. If a reaction does occur, write a balanced equation for it.

a. Can MnO₄ ^– ions oxidise Cl^– ions to Cl₂ in acidic conditions?

b. Can MnO₄^– ions oxidise F^– ions to F₂ in acidic conditions?

c. Can H⁺ ions oxidise V²⁺ ions to V³⁺ ions?

d. Can H⁺ ions oxidise Fe²⁺ ions to Fe³⁺ ions?

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Selected standard electrode potentials Electrode reaction E/V Electrode reactlon Ag* +e- Ag Mn2+ + 2e= Mn +0.80 -1.18 Br, + 2e 2Br Mno, + 8H* + 5e Mn2+ + 4H,0 +1.52 +1.07 Ca2+ + 2e Ca -2.87 Ni24 + 2e NI -0.25 Cl, + 2e - 201 NO, + 2H* + e - NO, + H,0 +1.36 +0.81 CIO + H,0 + 2e"= - Cl+ 20H- NO, + 10H* + 8e" NH,* +3H,0 +0.89 +0.87 Cr2+ + 2e Cr -0.91 0,+4H* + 4e 2H,0 +1.23 Cr3+ + 3e Cr 0,+ 2H,0+ 4e= 40H- -0.74 +0.40 Cr,0,7 +14H* + 6e 2Cr* + 7H,0 Pb2+ + 2e Pb -0.13 +1.33 Cut +e Cu Pbo, + 4H* + 2e - Pb2+ + +1.47 +0.52 Cu2+ +e= Cut +0.15 Snt + 2e Sn -0.14 Cu2+ + 2e Cu Sn+ + 2e Sn2+ +0.34 +0.15 F,+ 2e"- 2F- so + 4H* + 2e = so, + 2H,0 +0.17 +2.87 Fe2+ + 2e Fe -0.44 s,0,2 +2e- 25o, +2.01 Fe+ +e Fe2+ 5,0,2- + 2e= 25,0, +0.77 +0.09 Fe+ + 3e Fe -0.04 V2+ + 2e= V -1.20 2H* + 2e H, V3+ +e- V2+ 0.00 -0.26 2H,0 +2e VO2+ + 2H* +e V3+ + H,0 H, +20H- -0.83 +0.34 H,0, + 2H* + 2e - 2H,0 vo,* + 2H* +e= vo2* + H,0 +1.77 +1.00 I + 2e 21- vo,, + 4H* +e= vo2+ + 2H,0 +0.54 +1.00 K* +e= K -2.92 Zn2+ + 2e Zn -0.76 Mg2+ + 2e= Mg -2.38