Question

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
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

Use the tabulated electrode potentials to calculate K for the oxidation of zinc by H+:

Zn(s)+2H+(aq)→Zn2+(aq)+H2(g)

D)

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

Use tabulated standard electrode potentials to calculate the standard cell potential for the reaction occurring in an electrochemical cell at 25 ∘C. (The equation is balanced.)

Sn2+(aq)+Cd(s)→Sn(s)+Cd2+(aq)

E)

Balance the following redox reactions occurring in acidic aqueous solution.

MnO−4(aq)+Al(s) → Mn2+(aq)+Al3+(aq)

Answer 1