Salt bridge A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+ concentrations. The left compartment contains 0.341 M Cu2+ , and the right compartment contains 0.476 M Cu²+. Calculate the cell potential for this reaction at 298 K. volts In this copper concentration cell, the compartment on the left is the and the compartment on the anode right is the cathode Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) F2(g) + 2 e→2 F(aq) 2.87 Ce4*(aq) + e –→ Ce"(aq) 3+ 1.61 2+ MnO4 (aq) + 8 H"(aq) + 5 e¯ –→ Mn-T(aq) + 4 H2O(1) 1.51 Cl2(g) + 2 e' —2 СГ (aq) 1.36 Cr2072"(aq) + 14 H*(aq) + 6 e¯ →2 Cr"(aq) + 7 H2O(1) 1.33 O2(g) + 4 H*(aq) + 4 e→2 H2O(1) 1.229 Br2(1) + 2 e¯ –→2 Br¯(aq) 1.08 NO3 (aq) + 4 H"(aq) +3 e¯ –→ NO(g) + 2 H2O(1) 0.96 2 Hg-*(aq) + 2 e¯ → Hg22 (aq) 0.920 Hg-"(aq) + 2 e →Hg(1) 0.855 Ag"(aq) + e¯ – Ag(s) 0.799 2+, Hg2"(aq) + 2 e¯ →2 Hg(1) 0.789 Fe*(aq) + e → Fe2*(aq) 0.771 I2(s) + 2 e → 2 1 (aq) 0.535 Fe(CN)6° (aq) + e→ Fe(CN)64 (aq) 0.48 Cu2*(aq) + 2 e → Cu(s) 0.337 Cu2*(aq) + e" – Cu"(aq) 0.153 S(s) + 2 H*(aq) + 2 e → H2S(aq) 0.14 2 H*(aq) + 2 e → H2(g) 0.0000 Pb2*(aq) + 2 e → Pb(s) -0.126 Sn-"(aq) + 2 e¯ → Sn(s) „2+ -0.14 Ni2+(ag) + 2 e →Ni(s) -0.25 Co2+(ag) + 2 e →Co(s) -0.28 Cd2*(aq) + 2 e →Cd(s) -0.403 Cr3+ C* (aq) (aq) + e -0.41 Fe2*(aq) + 2 e →Fe(s) -0.44 Cr3+ (aq) + 3 e → Cr(s) -0.74 Zn2*(aq) + 2 e →Zn(s) -0.763 2 H20(1) + 2 e → H2(g) + 2 OH (aq) -0.83 Mn-"(aq) + 2 e¯ → Mn(s) 2+ -1.18 Als*(aq) + 3 e → Al(s) -1.66 2+ Mg"(aq) + 2 e →Mg(s) -2.37 Na"(aq) + e –→ Na(s) -2.714 K(aq) + e→ K(s) -2.925 Li*(aq) + e Li(s) -3.045
Salt bridge A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+ concentrations. The left compartment contains 0.341 M Cu2+ , and the right compartment contains 0.476 M Cu²+. Calculate the cell potential for this reaction at 298 K. volts In this copper concentration cell, the compartment on the left is the and the compartment on the anode right is the cathode Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) F2(g) + 2 e→2 F(aq) 2.87 Ce4*(aq) + e –→ Ce"(aq) 3+ 1.61 2+ MnO4 (aq) + 8 H"(aq) + 5 e¯ –→ Mn-T(aq) + 4 H2O(1) 1.51 Cl2(g) + 2 e' —2 СГ (aq) 1.36 Cr2072"(aq) + 14 H*(aq) + 6 e¯ →2 Cr"(aq) + 7 H2O(1) 1.33 O2(g) + 4 H*(aq) + 4 e→2 H2O(1) 1.229 Br2(1) + 2 e¯ –→2 Br¯(aq) 1.08 NO3 (aq) + 4 H"(aq) +3 e¯ –→ NO(g) + 2 H2O(1) 0.96 2 Hg-*(aq) + 2 e¯ → Hg22 (aq) 0.920 Hg-"(aq) + 2 e →Hg(1) 0.855 Ag"(aq) + e¯ – Ag(s) 0.799 2+, Hg2"(aq) + 2 e¯ →2 Hg(1) 0.789 Fe*(aq) + e → Fe2*(aq) 0.771 I2(s) + 2 e → 2 1 (aq) 0.535 Fe(CN)6° (aq) + e→ Fe(CN)64 (aq) 0.48 Cu2*(aq) + 2 e → Cu(s) 0.337 Cu2*(aq) + e" – Cu"(aq) 0.153 S(s) + 2 H*(aq) + 2 e → H2S(aq) 0.14 2 H*(aq) + 2 e → H2(g) 0.0000 Pb2*(aq) + 2 e → Pb(s) -0.126 Sn-"(aq) + 2 e¯ → Sn(s) „2+ -0.14 Ni2+(ag) + 2 e →Ni(s) -0.25 Co2+(ag) + 2 e →Co(s) -0.28 Cd2*(aq) + 2 e →Cd(s) -0.403 Cr3+ C* (aq) (aq) + e -0.41 Fe2*(aq) + 2 e →Fe(s) -0.44 Cr3+ (aq) + 3 e → Cr(s) -0.74 Zn2*(aq) + 2 e →Zn(s) -0.763 2 H20(1) + 2 e → H2(g) + 2 OH (aq) -0.83 Mn-"(aq) + 2 e¯ → Mn(s) 2+ -1.18 Als*(aq) + 3 e → Al(s) -1.66 2+ Mg"(aq) + 2 e →Mg(s) -2.37 Na"(aq) + e –→ Na(s) -2.714 K(aq) + e→ K(s) -2.925 Li*(aq) + e Li(s) -3.045
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Chapter1: Chemical Foundations
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Transcribed Image Text:Salt bridge
A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+
concentrations. The left compartment contains 0.341 M Cu2+ , and the right compartment contains 0.476 M
Cu²+.
Calculate the cell potential for this reaction at 298 K.
volts
In this copper concentration cell, the compartment on the left is the
and the compartment on the
anode
right is the
cathode
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C
Half-Cell Reaction
E° (volts)
F2(g) + 2 e→2 F(aq)
2.87
Ce4*(aq) + e –→ Ce"(aq)
3+
1.61
2+
MnO4 (aq) + 8 H"(aq) + 5 e¯ –→ Mn-T(aq) + 4 H2O(1)
1.51
Cl2(g) + 2 e' —2 СГ (aq)
1.36
Cr2072"(aq) + 14 H*(aq) + 6 e¯
→2 Cr"(aq) + 7 H2O(1)
1.33
O2(g) + 4 H*(aq) + 4 e→2 H2O(1)
1.229
Br2(1) + 2 e¯ –→2 Br¯(aq)
1.08
NO3 (aq) + 4 H"(aq) +3 e¯ –→ NO(g) + 2 H2O(1)
0.96
2 Hg-*(aq) + 2 e¯ →
Hg22 (aq)
0.920
Hg-"(aq) + 2 e →Hg(1)
0.855
Ag"(aq) + e¯ – Ag(s)
0.799
2+,
Hg2"(aq) + 2 e¯ →2 Hg(1)
0.789
Fe*(aq) + e →
Fe2*(aq)
0.771
I2(s) + 2 e → 2 1 (aq)
0.535
Fe(CN)6° (aq) + e→ Fe(CN)64 (aq)
0.48
Cu2*(aq) + 2 e → Cu(s)
0.337
Cu2*(aq) + e" – Cu"(aq)
0.153
S(s) + 2 H*(aq) + 2 e → H2S(aq)
0.14
2 H*(aq) + 2 e → H2(g)
0.0000
Pb2*(aq) + 2 e → Pb(s)
-0.126
Sn-"(aq) + 2 e¯ → Sn(s)
„2+
-0.14
Ni2+(ag) + 2 e →Ni(s)
-0.25
Co2+(ag) + 2 e →Co(s)
-0.28
Cd2*(aq) + 2 e →Cd(s)
-0.403
Cr3+
C* (aq)
(aq) + e
-0.41
Fe2*(aq) + 2 e →Fe(s)
-0.44
Cr3+
(aq) + 3 e → Cr(s)
-0.74
Zn2*(aq) + 2 e →Zn(s)
-0.763
2 H20(1) + 2 e → H2(g) + 2 OH (aq)
-0.83
Mn-"(aq) + 2 e¯ → Mn(s)
2+
-1.18
Als*(aq) + 3 e → Al(s)
-1.66
2+
Mg"(aq) + 2 e →Mg(s)
-2.37
Na"(aq) + e –→ Na(s)
-2.714
K(aq) + e→ K(s)
-2.925
Li*(aq) + e Li(s)
-3.045
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