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Which of the following redox reactions do you expect to occurspontaneously in the reverse direction?

Check all that apply:
1) 2Ag⁺(aq) + Ni(s) ------> 2Ag(s) + Ni²+(aq)

2) Fe(s) + Mn²⁺(aq) ------> Fe²⁺(aq) +Mn(s)

3) 2Al(s) + 3Pb²⁺(aq)-----> 2Al³⁺(aq)+3Pb(s)

4) Ca²⁺(aq) + Zn(s) -------> Ca(s) +Zn²⁺(aq)

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Related questions

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

Show transcribed image text Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy Î Go for the following redox reaction. Round your answer to 3 significant digits. 3Fe2 (aa)+Noj (a)+4H (aa)-3Fe (a)+ NO )+2H,00) 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

PLEASE INCLUDE CALCULATIONS

3. Suppose you have the following reagents available under standard conditions (i.e., P- 1 atm for all gases25 Â°C: C mol L1 for all aqueous species, including H.)

Co(s), Ag (aq), CI(aq), Cr(s), BrO3 (a), 2(s), F(aq)

Consult the standard reduction potentials on the next page and then answer the following questions

(a) Which is the strongest oxidizing agent?

(b) Which is the strongest reducing agent?

PLEASE INCLUDE CALCULATIONS/ FORMULAS

(c) Which of the available reagent(s), if any, will oxidize Cd(s) without oxidizing Pb(s)? If none of the available reagents can be used for this purpose, then identify another reagent from the table that could be used. For one of the reagents you've identified, write down a balanced chemical equation for the reaction that occurs.

Show transcribed image text

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