Calculate AG° and the equilibrium constant for the following reaction at 298 K:Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)Acidic SolutionStandard Electrode Potential, E (volts)H2O2(aq) + 2 H'(aq) + 2 eAu*(aq) + e- Au(s)Au (aq) + 3 e- Au(s)Br2(8) +2 e-→2 Br(aq)NO: (aq) + 4 H'(aq) + 3 e NO(g) + 2 H20Agʻ(aq) + e Ag(s)Hg2"(aq) + 2 eFe (aq) + e-- Fe2"(aq)Cu2*(aq) + 2 e Cu(s)HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq)Sn(aq) + 2e Sn2 (aq)2 H*(aq) + 2 e → Hz(g)Pb2*(aq) + 2 e Pb(s)Sn2"(aq) + 2 e Sn(s)Ni (aq) + 2 e → Ni(s)Cd2*(aq) + 2 e Cd(s)Cr (aq) + e - Cr*(aq)Fe2 (aq) + 2 e →Fe(s)Zn2*(aq) + 2 e Zn(s)Cr2*( aq) + 2 e Cr(s)Al3 (aq) + 3 e →Al(s)Mg2 (aq) + 2 e Mg(s)2 H20({)+1.77+1.68+1.50+1.08+0.96+0.802 Hg(8)+0.789+0.77+0.337+0.27+0.15 .0.00-0.126-0.14-0.25-0.40-0.408-0.44-0.763-0.91-1.66-2.37AG° =JK =

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Calculate AG° and the equilibrium constant for the following reaction at 298 K: 2+ Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)

Calculate AG° and the equilibrium constant for the following reaction at 298 K: 2+ Zn(aq) + Ni(s) → Zn(s) + Ni²(aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Calculate AG° and the equilibrium constant for the following reaction at 298 K:
Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)
Acidic Solution
Standard Electrode Potential, E (volts)
H2O2(aq) + 2 H'(aq) + 2 e
Au*(aq) + e- Au(s)
Au (aq) + 3 e- Au(s)
Br2(8) +2 e-→2 Br(aq)
NO: (aq) + 4 H'(aq) + 3 e NO(g) + 2 H20
Agʻ(aq) + e Ag(s)
Hg2"(aq) + 2 e
Fe (aq) + e-- Fe2"(aq)
Cu2*(aq) + 2 e Cu(s)
HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq)
Sn(aq) + 2e Sn2 (aq)
2 H*(aq) + 2 e → Hz(g)
Pb2*(aq) + 2 e Pb(s)
Sn2"(aq) + 2 e Sn(s)
Ni (aq) + 2 e → Ni(s)
Cd2*(aq) + 2 e Cd(s)
Cr (aq) + e - Cr*(aq)
Fe2 (aq) + 2 e →Fe(s)
Zn2*(aq) + 2 e Zn(s)
Cr2*( aq) + 2 e Cr(s)
Al3 (aq) + 3 e →Al(s)
Mg2 (aq) + 2 e Mg(s)
2 H20({)
+1.77
+1.68
+1.50
+1.08
+0.96
+0.80
2 Hg(8)
+0.789
+0.77
+0.337
+0.27
+0.15 .
0.00
-0.126
-0.14
-0.25
-0.40
-0.408
-0.44
-0.763
-0.91
-1.66
-2.37
AG° =
J
K =

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