Standard reduction potentials at 25°C NO3(aq)+4H+(aq) +3e¯→ NO(g) +2H2O(1) Na+ (aq)+eNa(s) Ni2+(aq)+2eNi(s) O2(g)+2H+(aq) + 2e¯ → H₂O2(aq) O2(g)+4H+(aq) +4e¯ → 2H2O(l) 0.957 -2.71 -0.257 0.695 1.229 O2(g)+2H2O(1)+4e¯→ 40H¯(aq) 0.401 03(g)+2H+(aq)+2e¯ → O2(g)+H2O(1) 2.076 Pb2+(aq)+2e Pb(s) -0.126 PbO2(s)+4H+(aq)+SO4²¯(aq) + 2e¯ → PbSO4(s)+2H2O(1) 1.691 PbSO4(s)+H+(aq) + 2e¯→ Pb(s)+HSO4¯(aq) -0.359 HSO4 (aq)+3H+(aq)+2e¯→ H₂SO3(aq) + H2O(l) 0.172 SO4(aq)+4H+(aq) + 2e¯-SO2(g) +2H2O(1) 0.172 Sc3+(aq)+3eSc(s) Sn2+(aq)+2e-Sn(s) Sn+(aq)+2e-Sn2+(aq) Sr2+(aq)+2e Sr(s) VO2+(aq)+2H+(aq)+e¯ → VO²+(aq)+H2O(l) Zn2+(aq)+2eZn(s) Standard reduction potentials at 25°C 2103 (aq)+12H+ (aq) +10e¯-12(s)+6H2O(1) K+(aq)+eK(s) Li+(aq)+eLi(s) -2.077 -0.138 0.151 -2.899 0.991 -0.762 1.195 -2.931 -3.040 Mg2+(aq)+2e-Mg(s) -2.372 Mn2+(aq)+2eMn(s) MnO2(s)+4H+(aq) + 2e¯- Mn2+(aq)+2H2O(1) MnO4 (aq)+8H+(aq) +5e¯ → Mn2+(aq)+4H₂O(1) -1.185 1.224 1.507 MnO4 (aq)+2H2O(l)+3e → MnO2(s)+40H¯(aq) 0.595 HNO2(aq)+H+(aq) +e¯-NO(g) + H2O(1) 0.983 N2(g)+5H+(aq)+4e¯ → N₂H5+(aq) -0.214 N2(g)+4H2O(1)+4e¯ →4OH¯(aq)+N2H4(aq) -1.16 NO3(aq)+4H+(aq)+3e¯ → NO(g)+2H2O(1) 0.957 Na+ (aq)+eNa(s) -2.71 Ni2+(aq)+2e-Ni(s) -0.257 O2(g)+2H+(aq) + 2e¯→ H₂O2(aq) 0.695 1.229 0.401 O2(g)+4H+(aq)+4e¯ + 2H2O(1) O2(g)+2H2O(1)+4e¯→ 40H¯(aq) oo Standard reduction potentials at 25°C Cr3+(aq)+3eCr(s) CrO4(aq)+4H2O(1)+3e¯→ Cr(OH)3(s)+50H¯(aq) Cr2O72(aq)+14H+(aq)+6e¯ → 2Cr³+(aq)+7H₂O(1) Cu+(aq)+e Cu(s) -0.744 -0.13 1.36 0.521 Cu2+(aq)+e Cu+(aq) 0.153 Cu2+(aq)+2eCu(s) 0.342 F2(g)+2e2F (aq) 2.866 Fe2+(aq) + 2e-Fe(s) -0.447 Fe3+(aq) +e-Fe²+(aq) 0.771 Fe3+(aq)+3e → Fe(s) -0.037 2H+(aq)+2e H2(g) 0.000 2H2O(1)+2e → H2(g)+20H¯(aq) -0.828 H2O2(aq)+2H+(aq) + 2e¯→ 2H2O(1) 1.776 Hg2+(aq) + 2e-Hg(1) 0.851 2Hg2+(aq)+2eHg2²+(aq) 0.92 Hg2+(aq)+2e2Hg(1) 0.797 0.536 12(s)+2e21¯(aq) o Standard reduction potentials at 25°C Alphabetical order E° order half-reaction E°(V) Ag+(aq)+e-Ag(s) 0.800 Al3+(aq)+3e Al(s) -1.676 Au+(aq) +e-Au(s) 1.692 Au3+(aq)+3e-Au(s) 1.498 Ba2+(aq)+2e-Ba(s) -2.912 Be2+(aq)+2e-Be(s) -1.847 Br2(1)+2e2Br¯(aq) 1.066 Ca2+(aq)+2e-Ca(s) -2.868 Cd2+(aq)+2e-Cd(s) -0.403 Ce+(aq)+e→Ce3+(aq) 1.72 Cl2(g)+2e2CI¯(aq) 1.358 Co2+(aq)+2e-Co(s) -0.28 Co3+(aq) +e-Co²+(aq) 1.92 Cr²+(aq)+2e-Cr(s) -0.913 Cr3+(aq)+eCr²+(aq) -0.407 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. N₂H(aq) +40H(aq) + 2Br₁₂ (l) → N₂ (g)+4H₂O (1)+4Br˜¯ (aq) N. 2 kJ x10 X

Using standard reduction potentials from the ALEKS Deta tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. Cu (aq) + HNO₂ (aq) + H* (aq) → Cu² (aq) + NO(g) + H₂O (1) X

Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) Which species is the reducing agent? HCI H2 MgCl2 Mg

Consider the following redox reaction: 3Ag+ (aq) + Al(s) → 3Ag (s) + A1³+ (aq) If this reaction starts with 2.50 g of Al and the enough amount of Ag+, how much of electric charge could be generated? 4.28 x 104 C 8.94 × 10³ C 2.68 × 104 C 6.25 × 10³ C O 1.67 x 104 C