What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cr(s)|Cr**(0.25 M) || 12(s)| 1-(0.20 M)|Pt(s)

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What is the voltage of the following cell?
Use the Reduction Potential Table found in Chapter 17 notes.
Cr(s)|Cr³*(0.25 M) || |2(s)|1-(0.20 M)|Pt(s)
Transcribed Image Text:What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cr(s)|Cr³*(0.25 M) || |2(s)|1-(0.20 M)|Pt(s)
Table 19.1
Standard Reduction Potentials at 25°C*
Half-Reaction
E°(V)
F2(g) + 2e - 2F (aq)
O3(g) + 2H'(aq) + 2e O2(g) + H2O
Co3* (aq) + e Co?*(aq)
H2O2{aq) + 2H'(aq) + 2e¯ → 2H20
PbO2(s) + 4H*(aq) + So3 (aq) + 2e¯ → PbSO,(s) + 2H2O
Ce (aq) + e
Mno (aq) + 8H*(aq) + 5e Mn?*(aq) + 4H2O
Au (aq) + 3e → Au(s)
Cl2(9) + 2e¯
Cr20} (aq) + 14H*(aq) + 6e → 2Cr³*(aq) + 7H2O
MnO2(s) + 4H*(aq) + 2e
O29) + 4H*(aq) + 4e¯ →2H20
Br2(/) + 2e – 2B1¯(aq)
NO3 (aq) + 4H*(aq) + 3e¯ – NO(g) + 2H2O
2H9²* (aq) + 2e
Hg*(aq) + 2e
Ag*(aq) + e
Fe* (aq) + e → Fe2*(aq)
O2(g) + 2H*(aq) + 2e H2O2(aq)
MnO,(aq) + 2H20 + 3e¯ →MNO2(s) + 40H (aq)
12(s) + 2e-→ 21"(aq)
O2(g) + 2H2O + 4e → 40H¯(aq)
Cu2*(aq) + 2e
AgCl(s) + e" → Ag(s) + CI"(aq)
so3 (aq) + 4H*(aq) + 2e - SO2(g) + 2H2O
Cu2"(aq) + e¯→Cu*(aq)
Sna* (aq) + 2e
2H (aq) + 2e
Pb2*(aq) + 2e
Sn2*(aq) + 2e-
Ni2* (aq) + 2e
Co2*(aq) + 2e
PbSOa(s) + 2e™
Cd2"(aq) + 2e
Fe2* (aq) + 2e
Cr3* (aq) + 3e
Zn2* (aq) + 2e
+2.87
+2.07
+1.82
+1.77
+1.70
- Ce3* (aq)
+1.61
+1.51
+1.50
2C1"(aq)
+1.36
+1.33
→ Mn2 (aq) + 2H2O
+1.23
+1.23
+1.07
+0.96
Hg3* (aq)
→ 2Hg()
→ Ag(s)
+0.92
+0.85
+0.80
+0.77
+0.68
+0.59
+0.53
+0.40
» Cu(s)
+0.34
+0.22
+0.20
+0.15
Sn2*(aq)
H2(g)
Pb(s)
→ Sn(s)
+0.13
0.00
-0.13
-0.14
-0.25
Ni(s)
Co(s)
Pb(s) + SO3-(aq)
Cd(s)
Fe(s)
Cr(s)
→ Zn(s)
H2(g) + 20H (aq)
→ Mn(s)
Al(s)
-0.28
-0.31
-0.40
-0.44
-0.74
-0.76
--0.83
2H20 + 2e
Mn2" (aq) + 2e
Al3* (aq) + 3e
Be?* (aq) + 2e
Mg? *(aq) + 2e
Na* (aq) + e
Ca? (aq) + 2e Ca(s)
Sr2 (aq) + 2e
Ba?* (aq) + 2e Ba(s)
K'(aq) + e
Li* (aq) + e Li(s)
-1.18
-1.66
Be(s)
-1.85
-2.37
Mg(s)
Na(s)
-2.71
-2.87
→ Sr(s)
-2.89
-2.90
K(s)
-2.93
-3.05
* For all halt-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm tor gases These are the standard-state vakues
Increasing strength as oxidizing agent
Increasing strength as reducing agent
Transcribed Image Text:Table 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E°(V) F2(g) + 2e - 2F (aq) O3(g) + 2H'(aq) + 2e O2(g) + H2O Co3* (aq) + e Co?*(aq) H2O2{aq) + 2H'(aq) + 2e¯ → 2H20 PbO2(s) + 4H*(aq) + So3 (aq) + 2e¯ → PbSO,(s) + 2H2O Ce (aq) + e Mno (aq) + 8H*(aq) + 5e Mn?*(aq) + 4H2O Au (aq) + 3e → Au(s) Cl2(9) + 2e¯ Cr20} (aq) + 14H*(aq) + 6e → 2Cr³*(aq) + 7H2O MnO2(s) + 4H*(aq) + 2e O29) + 4H*(aq) + 4e¯ →2H20 Br2(/) + 2e – 2B1¯(aq) NO3 (aq) + 4H*(aq) + 3e¯ – NO(g) + 2H2O 2H9²* (aq) + 2e Hg*(aq) + 2e Ag*(aq) + e Fe* (aq) + e → Fe2*(aq) O2(g) + 2H*(aq) + 2e H2O2(aq) MnO,(aq) + 2H20 + 3e¯ →MNO2(s) + 40H (aq) 12(s) + 2e-→ 21"(aq) O2(g) + 2H2O + 4e → 40H¯(aq) Cu2*(aq) + 2e AgCl(s) + e" → Ag(s) + CI"(aq) so3 (aq) + 4H*(aq) + 2e - SO2(g) + 2H2O Cu2"(aq) + e¯→Cu*(aq) Sna* (aq) + 2e 2H (aq) + 2e Pb2*(aq) + 2e Sn2*(aq) + 2e- Ni2* (aq) + 2e Co2*(aq) + 2e PbSOa(s) + 2e™ Cd2"(aq) + 2e Fe2* (aq) + 2e Cr3* (aq) + 3e Zn2* (aq) + 2e +2.87 +2.07 +1.82 +1.77 +1.70 - Ce3* (aq) +1.61 +1.51 +1.50 2C1"(aq) +1.36 +1.33 → Mn2 (aq) + 2H2O +1.23 +1.23 +1.07 +0.96 Hg3* (aq) → 2Hg() → Ag(s) +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 » Cu(s) +0.34 +0.22 +0.20 +0.15 Sn2*(aq) H2(g) Pb(s) → Sn(s) +0.13 0.00 -0.13 -0.14 -0.25 Ni(s) Co(s) Pb(s) + SO3-(aq) Cd(s) Fe(s) Cr(s) → Zn(s) H2(g) + 20H (aq) → Mn(s) Al(s) -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 --0.83 2H20 + 2e Mn2" (aq) + 2e Al3* (aq) + 3e Be?* (aq) + 2e Mg? *(aq) + 2e Na* (aq) + e Ca? (aq) + 2e Ca(s) Sr2 (aq) + 2e Ba?* (aq) + 2e Ba(s) K'(aq) + e Li* (aq) + e Li(s) -1.18 -1.66 Be(s) -1.85 -2.37 Mg(s) Na(s) -2.71 -2.87 → Sr(s) -2.89 -2.90 K(s) -2.93 -3.05 * For all halt-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm tor gases These are the standard-state vakues Increasing strength as oxidizing agent Increasing strength as reducing agent
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