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The half-reactions in a Galvanic cell are the following (ortheir reverse):

Sn⁴⁺(aq) + 2e^- ?Sn²⁺(aq) (E^o = 0.13 V) (I)

MnO₄^-(aq) + 8H⁺(aq) +5e^- ? Mn²⁺(aq) +4H₂O(l) (E^o = 1.51 V) (II)

(a) Select the reduction process that is more favorable. (b) Whatreaction occurs at the anode of the cell? (c) What reaction occursat the cathode? (d) Write a balanced equation for the overall cellreaction. (e) What is the standard cell potential?

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Casey DurganLv2

17 Dec 2019

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A Chemist designs a galvanic cell that uses two half reactions

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Show transcribed image text Using standard reduction potentials from the ALEKS Data tab calculate the standard reaction free energy AGO for the following redox reaction. Round your answer to 3 significant digits. N2 H (ag)+40H (aq)+2CI2 () N2 ()+4H20 (0)+4CI (aq) kJ
Half-Reaction 2.866 192 1.776 1692 1.507 1.498 1.35827 F2 (g)+2e >2F (aq) Co3+ (aq) + e-â Co2+ (aq) H2O2 (aq) + 2H+ (aq) + 2e-â 2H2O (1) Au+ (aq) + e-â Au (s) MnO4" (aq) + 8H+ (aq) + 5e-â Mn2+ (aq) + 4H2O (1) Au3+ (aq) + 3e-â Au (s) Cl2 (g) + 2e-â 2Cl-(aq) O2 (g)+4H+ (a)4e2H2O() MnO2 (s) + 4H+ (aq) + 2e-â Mn2+ (aq) + 2H2O (l) 21O3 (aq) +12H (aq)+10e2 (s) 6H20 () Br2)2e2Br (aq) VO2+ (aq) + 2H+ (aq) + e-â VO2+ (aq) + H2O (l) HNO2 (aq) + H+ (aq) + e-â NO (g) + H2O (l) NO3 (a) 4H+ (aq) 3e NO (g) 2H20 () Ag+ (aq) + e-â Ag (s) 1.229 1.224 1.195 1.066 0.991 0.983 0.957 0.7996
Fe3+ (aq)eFe2+ (acq) 02 (g) + 2H+ (aq) + 2e-â H2O2 (aq) MnO4 (aq) 2H2O ()3eMnO2 (s40H (aq) l2 (s)+ 2e 2 (aq) Cu (aq)Cu (s) 02 (g) + 2H2O (l) + 4e-â 4OH-(aq) Cu2+ (aq) +2e> Cu (s) HSO4 (aq)3Ht (aq)2eH2SO3 (aq)+ H2O (0) Cu2+ (aq) + e-â Cu+ (aq) Sn4+ (aq) + 2e-â Sn2+ (aq) 2H+ (aq) + 2e-â H2 (g) Fe3+ (aq) 3e Fe (s) Pb2+ (aq) + 2e-â Pb (s) CrO42-(aq)4H20( 3e Cr(OH)3 (s)+50H- (aq) Sn2+ (aq)+2e> Sn (s) Ni2+ (aq)+2eNi (s) Co2+ (aq) + 2e-â Co (s) PbSO4 (s) + H+ (aq) + 2e-â Pb (s) + HSO4-(aq) 0.695 0.595 0.5355 0.521 0.401 0.3419 0.172 0.153 0.151 0.000 -0.037 -0.1262 -0.13 -0.1375 -0.257 -0.28 -0.3588
CrO42-(aq)4H20(3e Cr(OH)3 (s)+50H- (aq) Sn2+ (aq)+2e> Sn (s) Ni2+ (aq) + 2e, Ni (s) Co2+ (aq) + 2e-â Co (s) PbSO4 (s)H (aq)2ePb (sHSO4 (aq) Cr3+ (aq) + e-â Cr2+ (aq) Fe2+ (aq) +2e Fe (s) Cr3+ (aq) + 3e-â Cr(s) Zn2+ (aq)+2e Zn (s) 2H20 () 2eH2 (g) + 20H (aq) Cr2+ (aq)+2e Cr (s) N2 (g) 4H2O)+4e 40H (aq) N2H4 (aq) Mn2+ (aq)+ 2e Mn (s) Al3+ (aq)+3e Al (s) Sc3+ (aq)3eSc (s) Mg2+ (aa)+ 2e Mg (s) Nat (aq)eNa (s) Ca2+ (aq) + 2e-â Ca (s) Ba2+ (aq) + 2e-â Ba (s) -0.13 0.1375 -0.257 -0.28 0.3588 -0.407 -0.447 -0.744 0.7618 0.8277 -0.913 1.185 1.676 -2.077 2.372 2.71 2.868 2.912

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