Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 92QRT
Related questions
Question
Calculate for the given reaction (all concentrations 1M) and determine whether it will go spontaneous or not: Ni +2Ag+ ↔ Ni+2+2Ag
![AuCl, (aq) + 3e
Br2(1) + 2e-
O2(g) + 4H*(aq) + 4e¯
MnO2(s) + 4H*(aq) + 2e¯
Cr20,2-(aq) + 14H*(aq) + 6e¯
Cl2(g) + 2e-
ClO;-(aq) + 6H*(aq) + 5e¯
Au³* (aq) + 3e-
MnO4-(aq) + 8H*(aq) + 5e¯
PbO2(s) + SO,²-(aq) + 4H*(aq) + 2e-
H2O2(aq) + 2H*(aq) + 2e¯
Со" (ag) + e
F2(g) + 2e¯«0
Au(s) + 4CI¯(aq)
►2B1¯(aq)
>2H20
→ Mn²+(aq) + 2H2O
→2Cr³*(aq) + 7H2O
→2CI^(aq)
→Cl2(g) + 3H2O
Au(s)
→Mn²*(aq) + 4H2O
→ PBSO4(s) + 2H2O
→2H20
→Co²*(aq)
2F¯(aq)
1.001
1.077
1.229
1.229
1.33
1.360
1.458
1.498
1.512
1.687
1.763
1.953
2.889
Basic Solution, [OH¯] = 1 M
E°red (V)
Fe(OH)2(s) + 2e
2H2O + 2e¯
Fe(OH)3(s) + e¯
S(s) + 2e-
NO;¯(aq) + 2H2O + 3e¯
NO;¯(aq) + H20 + 2e¯
ClO, (aq) + H2O + 2e¯
O2(g) + 2H2O + 4e¯
ClO;"(aq) + 3H2O + 6e¯
ClO-(aq) + H2O + 2e-
→Fe(s) + 20H¯(aq)
→H;(g) + 2OH¯(aq)
→Fe(OH)2(s) + OH (aq)
-0.891
-0.828
-0.547
-0.445
(bv)--S«
→NO(g) + 40H¯ (aq)
→NO, (aq) + 20H¯(aq)
→CIO; "(aq) + 2OH (aq)
→40H¯(aq)
→CIF(aq) + 6OH (aq)
→ClI[(aq) + 2OH¯(aq)
-0.140
0.004
0.398
0.401
0.614
0.890](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3ee82870-1f5d-43d4-bcac-0c5f3d14ca8b%2F46149507-a132-473a-8104-b7aa44877538%2Fx1373li_processed.png&w=3840&q=75)
Transcribed Image Text:AuCl, (aq) + 3e
Br2(1) + 2e-
O2(g) + 4H*(aq) + 4e¯
MnO2(s) + 4H*(aq) + 2e¯
Cr20,2-(aq) + 14H*(aq) + 6e¯
Cl2(g) + 2e-
ClO;-(aq) + 6H*(aq) + 5e¯
Au³* (aq) + 3e-
MnO4-(aq) + 8H*(aq) + 5e¯
PbO2(s) + SO,²-(aq) + 4H*(aq) + 2e-
H2O2(aq) + 2H*(aq) + 2e¯
Со" (ag) + e
F2(g) + 2e¯«0
Au(s) + 4CI¯(aq)
►2B1¯(aq)
>2H20
→ Mn²+(aq) + 2H2O
→2Cr³*(aq) + 7H2O
→2CI^(aq)
→Cl2(g) + 3H2O
Au(s)
→Mn²*(aq) + 4H2O
→ PBSO4(s) + 2H2O
→2H20
→Co²*(aq)
2F¯(aq)
1.001
1.077
1.229
1.229
1.33
1.360
1.458
1.498
1.512
1.687
1.763
1.953
2.889
Basic Solution, [OH¯] = 1 M
E°red (V)
Fe(OH)2(s) + 2e
2H2O + 2e¯
Fe(OH)3(s) + e¯
S(s) + 2e-
NO;¯(aq) + 2H2O + 3e¯
NO;¯(aq) + H20 + 2e¯
ClO, (aq) + H2O + 2e¯
O2(g) + 2H2O + 4e¯
ClO;"(aq) + 3H2O + 6e¯
ClO-(aq) + H2O + 2e-
→Fe(s) + 20H¯(aq)
→H;(g) + 2OH¯(aq)
→Fe(OH)2(s) + OH (aq)
-0.891
-0.828
-0.547
-0.445
(bv)--S«
→NO(g) + 40H¯ (aq)
→NO, (aq) + 20H¯(aq)
→CIO; "(aq) + 2OH (aq)
→40H¯(aq)
→CIF(aq) + 6OH (aq)
→ClI[(aq) + 2OH¯(aq)
-0.140
0.004
0.398
0.401
0.614
0.890
![Table 17.1 Standard Potentials in Water Solution at 25°C
Acidic Solution, [H*] = 1 M
E°red (V)
Li*(aq) + e-
K*(aq) + e-
Ba2+(aq) + 2e-
Ca2*(aq) + 2e¯
Na*(ag) + e
Mg2*(aq) + 2e-
Al3* (aq) + 3e
Mn²* (aq) + 2e-
Zn²* (aq) + 2e¯
Cr*(aq) + 3e-
Fe2* (aq) + 2e
Cr* (aq) + e¯
Cd2* (aq) + 2e-
PbSO4(s) + 2e-
→Li(s)«O
→K(s)
→Ba(s)
Ca(s)
►Na(s)
►Mg(s)
→Al(s)
→Mn(s)
-3.040
-2.936
-2.906
-2.869
-2.714
-2.357
-1.68
-1.182
→Zn(s)
→Cr(s)
► Fe(s)
→C²*(aq)
→Cd(s)
►Pb(s) + SO,²-(aq)
→ Tl(s)
→Co(s)
→Ni(s)
→ Ag(s) + I-(aq)
► Sn(s)
→Pb(s)
→H2(g)
► Ag(s) + Br¯(aq)
→H;S(aq)
► Sn²+(aq)
→SO2(g) + 2H¿O
►Cu*(aq)
►Cu(s)
-0.762
-0.744
-0.409
-0.408
-0.402
-0.356
TI*(aq) + e
Co*(aq) + 2e
Ni2*(aq) + 2e
AgI(s) + e-
Sn²* (aq) + 2e-
Pb²*(aq) + 2e-
2H*(aq) + 2e
AgBr(s) + e-
S(s) + 2H*(aq) + 2e-
Sn**(aq) + 2e-
SO,?-(aq) + 4H* (aq) + 2e¯
Cu²*(aq) + e¯
Cu2* (aq) + 2e-
Cu*(aq) + e-
I2(s) + 2e-
Fe*(aq) + e
Hg,2* (aq) + 2e¯
Ag*(aq) + e-
2Hg²*(aq) + 2e
NO, lag) + 4H*(ag) + 3e-
-0.336
-0.282
-0.236
-0.152
-0.141
-0.127
0.000
0.073
0.144
0.154
0.155
0.161
0.339
0.518
0.534
Cu(s)
►21¬(aq)
→Fe²*(aq)
→2Hg(l)
► Ag(s)
→Hg;²*(aq)
0.769
0.796
0.799
0.908
►NO(g) + 2H,O
0.964
Increasing strength of oxidizing agents
Increasing strength of reducing agents](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3ee82870-1f5d-43d4-bcac-0c5f3d14ca8b%2F46149507-a132-473a-8104-b7aa44877538%2Fodnduaw_processed.png&w=3840&q=75)
Transcribed Image Text:Table 17.1 Standard Potentials in Water Solution at 25°C
Acidic Solution, [H*] = 1 M
E°red (V)
Li*(aq) + e-
K*(aq) + e-
Ba2+(aq) + 2e-
Ca2*(aq) + 2e¯
Na*(ag) + e
Mg2*(aq) + 2e-
Al3* (aq) + 3e
Mn²* (aq) + 2e-
Zn²* (aq) + 2e¯
Cr*(aq) + 3e-
Fe2* (aq) + 2e
Cr* (aq) + e¯
Cd2* (aq) + 2e-
PbSO4(s) + 2e-
→Li(s)«O
→K(s)
→Ba(s)
Ca(s)
►Na(s)
►Mg(s)
→Al(s)
→Mn(s)
-3.040
-2.936
-2.906
-2.869
-2.714
-2.357
-1.68
-1.182
→Zn(s)
→Cr(s)
► Fe(s)
→C²*(aq)
→Cd(s)
►Pb(s) + SO,²-(aq)
→ Tl(s)
→Co(s)
→Ni(s)
→ Ag(s) + I-(aq)
► Sn(s)
→Pb(s)
→H2(g)
► Ag(s) + Br¯(aq)
→H;S(aq)
► Sn²+(aq)
→SO2(g) + 2H¿O
►Cu*(aq)
►Cu(s)
-0.762
-0.744
-0.409
-0.408
-0.402
-0.356
TI*(aq) + e
Co*(aq) + 2e
Ni2*(aq) + 2e
AgI(s) + e-
Sn²* (aq) + 2e-
Pb²*(aq) + 2e-
2H*(aq) + 2e
AgBr(s) + e-
S(s) + 2H*(aq) + 2e-
Sn**(aq) + 2e-
SO,?-(aq) + 4H* (aq) + 2e¯
Cu²*(aq) + e¯
Cu2* (aq) + 2e-
Cu*(aq) + e-
I2(s) + 2e-
Fe*(aq) + e
Hg,2* (aq) + 2e¯
Ag*(aq) + e-
2Hg²*(aq) + 2e
NO, lag) + 4H*(ag) + 3e-
-0.336
-0.282
-0.236
-0.152
-0.141
-0.127
0.000
0.073
0.144
0.154
0.155
0.161
0.339
0.518
0.534
Cu(s)
►21¬(aq)
→Fe²*(aq)
→2Hg(l)
► Ag(s)
→Hg;²*(aq)
0.769
0.796
0.799
0.908
►NO(g) + 2H,O
0.964
Increasing strength of oxidizing agents
Increasing strength of reducing agents
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