Using the provided table, calculate AG° at 298 K for the following reaction: Zn²(aq) + 21(aq) Zn(s) + I:(s) TABLE 18.1 Standard Reduction Potentials in Water at 25°C Potential (V) Reduction Half-Reaction F2(g) + 2 e¯ –→ 2 F"(aq) MnO,¯(aq) + 8 H*(aq) + 5 e¯ → Mn²*(aq) + 4 H2O(I) Cl2(g) + 2 e¯ 2 CI^(aq) CrO,²-(aq) + 14 H*(aq) + 6 e¯ → 2 Cr³*(aq) + 7 H2O(I) O-{g) + 4 H*(aq) + 4 e¯ → 2 H¿O(I) Br2(1) + 2 e¯ –→ 2 Br¯(aq) NO3"(aq) + 4 H*(aq) + 3 e¯ → NO(g) + 2 H¿O(I) Ag*(aq) + e¯ – Ag(s) Fe*(aq) + e¯ → Fe²*(aq) O2(8) + 2 H*(aq) + 2 e¯ → HO2(aq) MnO4¯(aq) + 2 H2O(1) + 3 e¯ – MnO2(s) + 4 OH¯(aq) I(s) + 2 e¯ – 21°(aq) O2(g) + 2 H¿O(I) + 4 e¯ → Cu²*(aq) + 2 e¯ 2H*(aq) + 2 e¯ → H2(g) Ni²*(aq) + 2 e¯ Fe*(aq) + 2 e¯ Zn²*(aq) + 2 e¯ +2.87 +1.51 +1.36 +1.33 +1.23 +1.06 +0.96 +0.80 +0.77 +0.68 +0.59 +0.54 +0.40 4 OH"(aq) +0.34 Cu(s) 0 [defined] -0.28 • Ni(s) -0.44 Fe(s) Zn(s) -0.76 H2(g) + 2 OH¯(aq) Al(s) 2 H¿O(1) + 2 e¯ Al³*(aq) + 3 e¯ Na*(aq) + e¯ → Na(s) Li*(aq) + e¯ – Li(s) -0.83 -1.66 -2.71 -3.05 а. -125.5 kJ/mol b. -250.9 kJ/mol C. 125.5 kJ/mol d. 250.9 kJ/mol
Using the provided table, calculate AG° at 298 K for the following reaction: Zn²(aq) + 21(aq) Zn(s) + I:(s) TABLE 18.1 Standard Reduction Potentials in Water at 25°C Potential (V) Reduction Half-Reaction F2(g) + 2 e¯ –→ 2 F"(aq) MnO,¯(aq) + 8 H*(aq) + 5 e¯ → Mn²*(aq) + 4 H2O(I) Cl2(g) + 2 e¯ 2 CI^(aq) CrO,²-(aq) + 14 H*(aq) + 6 e¯ → 2 Cr³*(aq) + 7 H2O(I) O-{g) + 4 H*(aq) + 4 e¯ → 2 H¿O(I) Br2(1) + 2 e¯ –→ 2 Br¯(aq) NO3"(aq) + 4 H*(aq) + 3 e¯ → NO(g) + 2 H¿O(I) Ag*(aq) + e¯ – Ag(s) Fe*(aq) + e¯ → Fe²*(aq) O2(8) + 2 H*(aq) + 2 e¯ → HO2(aq) MnO4¯(aq) + 2 H2O(1) + 3 e¯ – MnO2(s) + 4 OH¯(aq) I(s) + 2 e¯ – 21°(aq) O2(g) + 2 H¿O(I) + 4 e¯ → Cu²*(aq) + 2 e¯ 2H*(aq) + 2 e¯ → H2(g) Ni²*(aq) + 2 e¯ Fe*(aq) + 2 e¯ Zn²*(aq) + 2 e¯ +2.87 +1.51 +1.36 +1.33 +1.23 +1.06 +0.96 +0.80 +0.77 +0.68 +0.59 +0.54 +0.40 4 OH"(aq) +0.34 Cu(s) 0 [defined] -0.28 • Ni(s) -0.44 Fe(s) Zn(s) -0.76 H2(g) + 2 OH¯(aq) Al(s) 2 H¿O(1) + 2 e¯ Al³*(aq) + 3 e¯ Na*(aq) + e¯ → Na(s) Li*(aq) + e¯ – Li(s) -0.83 -1.66 -2.71 -3.05 а. -125.5 kJ/mol b. -250.9 kJ/mol C. 125.5 kJ/mol d. 250.9 kJ/mol
General Chemistry - Standalone book (MindTap Course List)
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ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.148QP: Consider the following cell reaction at 25C. 2Cr(s)+3Fe2+(aq)2Cr3+(aq)+3Fe(s) Calculate the standard...
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![Using the provided table, calculate AG° at 298 K for the following reaction:
Zn² (aq) + 21(aq) → Zn(s) + I:(s)
TABLE 18.1 Standard Reduction Potentials in Water at 25°C
Potential (V)
Reduction Half-Reaction
+2.87
F2(g) + 2 e¯ –→ 2 F (aq)
MnO,¯(aq) + 8 H*(aq) + 5 e¯
Cl2(g) + 2 e¯ –→ 2 CI^(aq)
Cr,O,²~(aq) + 14 H*(aq) + 6 e¯ → 2 Cr³*(aq) + 7 H2O(1)
O2(g) + 4 H*(aq) + 4 e¯ → 2 H2O(1)
Br2(1) + 2 e¯ – 2 Br¯(aq)
NO3¯(aq) + 4 H*(aq) + 3 e¯ → NO(g) + 2 H2O(1)
Ag*(aq) + e¯ – Ag(s)
Fe*(aq) + e¯
O2(g) + 2 H*(aq) + 2 e¯ → H2O2(aq)
MnO,"(aq) + 2 H2O(I) + 3 e¯ – MnO2(s) + 4 OH¯(aq)
I2(s) + 2 e¯ 21 (aq)
O2(g) + 2 H2O(I) + 4 e¯ → 4 OH¯(aq)
Cu²*(aq) + 2 e¯
2 H*(aq) + 2 e¯ → H2(g)
Ni*(aq) + 2 e → Ni(s)
Fe2*(aq) + 2 e → Fe(s)
Zn2*(aq) + 2 e¯ → Zn(s)
+1.51
Mn2*(aq) + 4 H2O(1)
+1.36
+1.33
+1.23
+1.06
+0.96
+0.80
+0.77
Fe2*(aq)
+0.68
+0.59
+0.54
+0.40
+0.34
Cu(s)
0 [defined]
-0.28
-0.44
-0.76
2 H2O(1) + 2 e¯
Al3*(aq) + 3 e → Al(s)
Na*(aq) + e¯ – Na(s)
Li*(aq) + e¯ –→ Li(s)
-0.83
H2(g) + 2 OH¯(aq)
-1.66
-2.71
-3.05
а.
-125.5 kJ/mol
b.
-250.9 kJ/mol
С.
125.5 kJ/mol
d.
250.9 kJ/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6cb3e0c-030d-4f66-83a1-3a43f22b53c1%2F3b3d1819-9f3a-420b-b381-059923365549%2Fom8f8sg_processed.png&w=3840&q=75)
Transcribed Image Text:Using the provided table, calculate AG° at 298 K for the following reaction:
Zn² (aq) + 21(aq) → Zn(s) + I:(s)
TABLE 18.1 Standard Reduction Potentials in Water at 25°C
Potential (V)
Reduction Half-Reaction
+2.87
F2(g) + 2 e¯ –→ 2 F (aq)
MnO,¯(aq) + 8 H*(aq) + 5 e¯
Cl2(g) + 2 e¯ –→ 2 CI^(aq)
Cr,O,²~(aq) + 14 H*(aq) + 6 e¯ → 2 Cr³*(aq) + 7 H2O(1)
O2(g) + 4 H*(aq) + 4 e¯ → 2 H2O(1)
Br2(1) + 2 e¯ – 2 Br¯(aq)
NO3¯(aq) + 4 H*(aq) + 3 e¯ → NO(g) + 2 H2O(1)
Ag*(aq) + e¯ – Ag(s)
Fe*(aq) + e¯
O2(g) + 2 H*(aq) + 2 e¯ → H2O2(aq)
MnO,"(aq) + 2 H2O(I) + 3 e¯ – MnO2(s) + 4 OH¯(aq)
I2(s) + 2 e¯ 21 (aq)
O2(g) + 2 H2O(I) + 4 e¯ → 4 OH¯(aq)
Cu²*(aq) + 2 e¯
2 H*(aq) + 2 e¯ → H2(g)
Ni*(aq) + 2 e → Ni(s)
Fe2*(aq) + 2 e → Fe(s)
Zn2*(aq) + 2 e¯ → Zn(s)
+1.51
Mn2*(aq) + 4 H2O(1)
+1.36
+1.33
+1.23
+1.06
+0.96
+0.80
+0.77
Fe2*(aq)
+0.68
+0.59
+0.54
+0.40
+0.34
Cu(s)
0 [defined]
-0.28
-0.44
-0.76
2 H2O(1) + 2 e¯
Al3*(aq) + 3 e → Al(s)
Na*(aq) + e¯ – Na(s)
Li*(aq) + e¯ –→ Li(s)
-0.83
H2(g) + 2 OH¯(aq)
-1.66
-2.71
-3.05
а.
-125.5 kJ/mol
b.
-250.9 kJ/mol
С.
125.5 kJ/mol
d.
250.9 kJ/mol
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