Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures.
Standard reduction half-cell potentials at 25∘C
Half-reaction | E∘ (V) | Half-reaction | E∘ (V) | |
Au3+(aq)+3e−→Au(s) | 1.50 | Fe2+(aq)+2e−→Fe(s) | −0.45 | |
Ag+(aq)+e−→Ag(s) | 0.80 | Cr3+(aq)+e−→Cr2+(aq) | −0.50 | |
Fe3+(aq)+3e−→Fe2+(aq) | 0.77 | Cr3+(aq)+3e−→Cr(s) | −0.73 | |
Cu+(aq)+e−→Cu(s) | 0.52 | Zn2+(aq)+2e−→Zn(s) | −0.76 | |
Cu2+(aq)+2e−→Cu(s) | 0.34 | Mn2+(aq)+2e−→Mn(s) | −1.18 | |
2H+(aq)+2e−→H2(g) | 0.00 | Al3+(aq)+3e−→Al(s) | −1.66 | |
Fe3+(aq)+3e−→Fe(s) | −0.036 | Mg2+(aq)+2e−→Mg(s) | −2.37 | |
Pb2+(aq)+2e−→Pb(s) | −0.13 | Na+(aq)+e−→Na(s) | −2.71 | |
Sn2+(aq)+2e−→Sn(s) | −0.14 | Ca2+(aq)+2e−→Ca(s) | −2.76 | |
Ni2+(aq)+2e−→Ni(s) | −0.23 | Ba2+(aq)+2e−→Ba(s) | −2.90 | |
Co2+(aq)+2e−→Co(s) | −0.28 | K+(aq)+e−→K(s) | −2.92 | |
Cd2+(aq)+2e−→Cd(s) | −0.40 | Li+(aq)+e−→Li(s) | −3.04 |
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Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g)...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73 0.52 -0.76 0.34 -1.18 Half-reaction Aut (aq) + 3e +Au(s) Ag+ (aq) + +Ag(s) Fe3+ (aq) +34 Fo+ (aq) Cut(aq) + Cu(s) Cu²+ (aq) + 2e +Cu(s) 2H+ (aq) - 2e +H2 (6) Fe3+ (aq) + 3e Fe(s) Pb2+ (aq) + 2e →Pb(s) Sn-(aq) + 2e +Sn(s) Ni2+ (aq) + 2e →Ni(s) Co2(aq) +2e + Co(s) ca? (aq) + 2e +Cd(s) 0.00 Half-reaction Fe(aq)...
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an electrochemical cell at 25 C. (The equation is balanced.) 3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq) Express your answer to two significant figures and include the appropriate units. em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
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