Selected Standard Reduction Potentials at 25 °C Half-Reaction E° (V) Hg2 2+(aq) + 2e- 2Hg(l) +0.7973 Fe*(aq) + e¯ Fe2+(aq) +0.771 MnO4 (aq) + 2H,0(1) + 3e¯ MnO2(s) + 40H¯(aq) +0.558 I2(s) + 2e¯ 21 (aq) +0.5355 NiO2(s) + 2H2O(1) + 2e¬ Ni(OH)2(s) + 20H¯(aq) +0.49 Cu*(aq) + 2e¯ → Cu(s) +0.34 Hg2 Cl2(s) + 2e- 2Hg(1) + 2C1¯(aq) +0.26808 AgCl(s) + e¯ Ag(s)+ Cl¯(aq) +0.22233 Sn**(aq) + 2e¯ 4+ Sn²*(aq) 2+ +0.151 2H*(aq) + 2e¯ H2(8) 0.00 РЬ2 "(aq) + 2e - → Pb(s) -0.1262 Sn2+(aq) + 2e Sn(s) -0.1375 Ni2+(ag) + 2e¯ → Ni(s) -0.257 Co+(ag) + 2e¯ → Co(s) -0.28 PBSO4(s) + 2e¯ - Pb(s) + S04²(aq) -0.3505 2+ Cd(ag) + 2e¯ → Cd(s) -0.4030 Fe2+ (aq) + 2e¯ Fe(s) -0.447 Cr*(aq) + 3e¯ → Cr(s) -0.744 Mn²+(aq) + 2e- Mn(s) -1.185 Zn(OH)2(s) + 2e- Zn(s) + 20H¯(aq) -1.245 Zn2+(aq) + 2e¯ Zn(s) -0.7618 3+ Al*(aq) + 3e¬ → Al(s) -1.662 Mg (aq) + 2e¯ Mg(s) -2.372 Na *(aq) + e¯ Na(s) -2.71 Ca2+(aq) + 2e¯ → Ca(s) -2.868 Table 17.1 Selected Standard Reduction Potentials at 25 °C Half-Reaction E° (V) BaT(aq) + 2e¯ Ba(s) -2.912 к "aq) + е" K(s) -2.931 Li*(aq) +e¯ Li(s) -3.04 Table 17.1
Selected Standard Reduction Potentials at 25 °C Half-Reaction E° (V) Hg2 2+(aq) + 2e- 2Hg(l) +0.7973 Fe*(aq) + e¯ Fe2+(aq) +0.771 MnO4 (aq) + 2H,0(1) + 3e¯ MnO2(s) + 40H¯(aq) +0.558 I2(s) + 2e¯ 21 (aq) +0.5355 NiO2(s) + 2H2O(1) + 2e¬ Ni(OH)2(s) + 20H¯(aq) +0.49 Cu*(aq) + 2e¯ → Cu(s) +0.34 Hg2 Cl2(s) + 2e- 2Hg(1) + 2C1¯(aq) +0.26808 AgCl(s) + e¯ Ag(s)+ Cl¯(aq) +0.22233 Sn**(aq) + 2e¯ 4+ Sn²*(aq) 2+ +0.151 2H*(aq) + 2e¯ H2(8) 0.00 РЬ2 "(aq) + 2e - → Pb(s) -0.1262 Sn2+(aq) + 2e Sn(s) -0.1375 Ni2+(ag) + 2e¯ → Ni(s) -0.257 Co+(ag) + 2e¯ → Co(s) -0.28 PBSO4(s) + 2e¯ - Pb(s) + S04²(aq) -0.3505 2+ Cd(ag) + 2e¯ → Cd(s) -0.4030 Fe2+ (aq) + 2e¯ Fe(s) -0.447 Cr*(aq) + 3e¯ → Cr(s) -0.744 Mn²+(aq) + 2e- Mn(s) -1.185 Zn(OH)2(s) + 2e- Zn(s) + 20H¯(aq) -1.245 Zn2+(aq) + 2e¯ Zn(s) -0.7618 3+ Al*(aq) + 3e¬ → Al(s) -1.662 Mg (aq) + 2e¯ Mg(s) -2.372 Na *(aq) + e¯ Na(s) -2.71 Ca2+(aq) + 2e¯ → Ca(s) -2.868 Table 17.1 Selected Standard Reduction Potentials at 25 °C Half-Reaction E° (V) BaT(aq) + 2e¯ Ba(s) -2.912 к "aq) + е" K(s) -2.931 Li*(aq) +e¯ Li(s) -3.04 Table 17.1
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question. What is the standard cell potential (Eo), in volts, for the following voltaic cell? Type in your answer as a number to two decimal places with no units.
Al(s)|Al3+||Cr3+|Cr(s)
Transcribed Image Text:Selected Standard Reduction Potentials at 25 °C
Half-Reaction
E° (V)
Hg2 2+(aq) + 2e-
2Hg(l)
+0.7973
Fe*(aq) + e¯
Fe2+(aq)
+0.771
MnO4 (aq) + 2H,0(1) + 3e¯
MnO2(s) + 40H¯(aq)
+0.558
I2(s) + 2e¯
21 (aq)
+0.5355
NiO2(s) + 2H2O(1) + 2e¬
Ni(OH)2(s) + 20H¯(aq)
+0.49
Cu*(aq) + 2e¯ → Cu(s)
+0.34
Hg2 Cl2(s) + 2e-
2Hg(1) + 2C1¯(aq)
+0.26808
AgCl(s) + e¯
Ag(s)+ Cl¯(aq)
+0.22233
Sn**(aq) + 2e¯
4+
Sn²*(aq)
2+
+0.151
2H*(aq) + 2e¯
H2(8)
0.00
РЬ2
"(aq) + 2e - →
Pb(s)
-0.1262
Sn2+(aq) + 2e
Sn(s)
-0.1375
Ni2+(ag) + 2e¯ → Ni(s)
-0.257
Co+(ag) + 2e¯ → Co(s)
-0.28
PBSO4(s) + 2e¯
- Pb(s) + S04²(aq)
-0.3505
2+
Cd(ag) + 2e¯ → Cd(s)
-0.4030
Fe2+ (aq) + 2e¯
Fe(s)
-0.447
Cr*(aq) + 3e¯ → Cr(s)
-0.744
Mn²+(aq) + 2e-
Mn(s)
-1.185
Zn(OH)2(s) + 2e-
Zn(s) + 20H¯(aq)
-1.245
Zn2+(aq) + 2e¯
Zn(s)
-0.7618
3+
Al*(aq) + 3e¬ → Al(s)
-1.662
Mg (aq) + 2e¯
Mg(s)
-2.372
Na *(aq) + e¯
Na(s)
-2.71
Ca2+(aq) + 2e¯ → Ca(s)
-2.868
Table 17.1
Transcribed Image Text:Selected Standard Reduction Potentials at 25 °C
Half-Reaction
E° (V)
BaT(aq) + 2e¯
Ba(s)
-2.912
к "aq) + е"
K(s)
-2.931
Li*(aq) +e¯
Li(s)
-3.04
Table 17.1
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