spontaneous: [assume SHE value is zero] a) Pd (aq)2+ + H, (g) -à Pd (s) + 2H* (aq) b) Sn (aq)++ + H, (g) -à Sn(aq)2++ 2H* (aq) c) Ni (aq)2+ + H, (g) -à Ni (s) + 2H* (aq) d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq) Given Pd*/Pd =0.987 V, Snª*/ Sn²+ =0.154 V, Ni²+/Ni = -0.250 V, Cď*/Cd = -0.403 V From your answers, decide which of the above
spontaneous: [assume SHE value is zero] a) Pd (aq)2+ + H, (g) -à Pd (s) + 2H* (aq) b) Sn (aq)++ + H, (g) -à Sn(aq)2++ 2H* (aq) c) Ni (aq)2+ + H, (g) -à Ni (s) + 2H* (aq) d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq) Given Pd*/Pd =0.987 V, Snª*/ Sn²+ =0.154 V, Ni²+/Ni = -0.250 V, Cď*/Cd = -0.403 V From your answers, decide which of the above
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter14: Acids And Bases
Section14.9: Lewis Acids And Bases
Problem 14.26E
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Question
![1. Predict whether the following reactions are
spontaneous: [assume SHE value is zero]
a) Pd (aq)?+ + H, (g) -à Pd (s) + 2H† (aq)
b) Sn (aq)++ + H, (g) -à Sn(aq)2+ + 2H* (aq)
c) Ni (aq)?* + H, (g) -à Ni (s) + 2H* (aq)
d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq)
Given Pd+/Pd =0.987 V, Snª*/ Sn²+ =0.154 V,
Ni²*/Ni = -0.250 V, Cď*/Cd = -0.403 V
From your answers, decide which of the above
metals/metal ion could be reduced by hydrogen.
2. Identify the oxidizing agents and reducing agents in
the above reaction (1.)
3. Using the standard potentials, Calculate E
and equilibrium constant for the following
two reactions:
→ 2 TI(s) + Cl,(g)
a) TI*(aq) + 2 C(aq)
given the following standard reduction potentials.
Cl,(g) + 2 e →
TI*(aq) + e →
E° = +1.36 V
2 Cl(aq)
TI(s)
E° = -0.34 V
5 Cd2+
b) 5 Cd(s) + 2 MnO,¯(aq) + 16 H*(aq)
(aq) + 2 Mn²*(aq) + 8 H,O(1); given the
following standard reduction potentials.
MnO4 (aq) + 8 H*(aq) + 5 e → Mn²*(aq) + 4
H,O1)
Сd+(aq) + 2 е —>
E° = +1.52 V
Cd(s)
E° = -0.40 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff27c3bcc-31ef-40b0-b008-4b23339d198c%2F15e94974-55fb-4c10-973b-8520a0a1bd6a%2F1ty62s9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. Predict whether the following reactions are
spontaneous: [assume SHE value is zero]
a) Pd (aq)?+ + H, (g) -à Pd (s) + 2H† (aq)
b) Sn (aq)++ + H, (g) -à Sn(aq)2+ + 2H* (aq)
c) Ni (aq)?* + H, (g) -à Ni (s) + 2H* (aq)
d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq)
Given Pd+/Pd =0.987 V, Snª*/ Sn²+ =0.154 V,
Ni²*/Ni = -0.250 V, Cď*/Cd = -0.403 V
From your answers, decide which of the above
metals/metal ion could be reduced by hydrogen.
2. Identify the oxidizing agents and reducing agents in
the above reaction (1.)
3. Using the standard potentials, Calculate E
and equilibrium constant for the following
two reactions:
→ 2 TI(s) + Cl,(g)
a) TI*(aq) + 2 C(aq)
given the following standard reduction potentials.
Cl,(g) + 2 e →
TI*(aq) + e →
E° = +1.36 V
2 Cl(aq)
TI(s)
E° = -0.34 V
5 Cd2+
b) 5 Cd(s) + 2 MnO,¯(aq) + 16 H*(aq)
(aq) + 2 Mn²*(aq) + 8 H,O(1); given the
following standard reduction potentials.
MnO4 (aq) + 8 H*(aq) + 5 e → Mn²*(aq) + 4
H,O1)
Сd+(aq) + 2 е —>
E° = +1.52 V
Cd(s)
E° = -0.40 V
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