1. Calculate AG and predict whether the following reaction would proceed spontaneously as written at 298K: 2+ Mg(s) + Sn²+ (aq) Mg²+ (aq) + Sn(s) given that [Mg2+]=0.045 M, [Sn²+]=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)
1. Calculate AG and predict whether the following reaction would proceed spontaneously as written at 298K: 2+ Mg(s) + Sn²+ (aq) Mg²+ (aq) + Sn(s) given that [Mg2+]=0.045 M, [Sn²+]=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter16: Spontaneity Of Reaction
Section: Chapter Questions
Problem 6QAP: On the basis of your experience, predict which of the following reactions are spontaneous. (a)...
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![Table 20.1 Standard reduction potentials at 25°C*
Increasing strength as oxidizing agent
Half-Reaction
Li*(aq) + e
K+ (aq) + e
Ba²+ (aq) + 2e
Sr²+ (aq) + 2e-
Ca²+ (aq) + 2e
Na + (aq) + e
Mg²+ (aq) + 2e
Be²+ (aq) + 2e
Al³+ (aq) + 3e
Mn²+ (aq) + 2e
2H₂O + 2e™
Zn²+ (aq) + 2e-
Cr³+ (aq) + 3e
Fe²+ (aq) + 2e
Cd²+ (aq) + 2e
PbSO4(s) + 2e
Co²+ (aq) + 2e
Ni²+ (aq) + 2e
2+
Sn²+ (aq) + 2e
Pb²+ (aq) + 2e
Li(s)
K(s)
Ba(s)
→ Sr(s)
Ca(s)
Na(s)
Mg(s)
Be(s)
Al(s)
→→ Mn(s)
H₂(g) + 2OH(aq)
Zn(s)
Cr(s)
Fe(s)
Cd(s)
Pb(s) +
Co(s)
Ni(s)
Sn(s)
Pb(s)
H₂(g)
Sn²+ (aq)
+ SO² (aq)
4+
2H¹ (aq) + 2e
Sn¹+ (aq) + 2e
Cu²+ (aq) + e
→ Cut (aq)
SO (aq) + 4H+ (aq) + 2e SO₂(g) + 2H₂O
AgCl(s) + e → Ag(s) + Cl(aq)
Cu²+ (aq) + 2e
Cu(s)
O₂(g) + 2H₂O + 4e¯¯ →
[₂ (s) + 2e →→→→→→→ 21 (aq)
MnO4 (aq) + 2H₂O + 3e -
O₂(g) + 2H+ (aq) + 2e¯
Fe²+ (aq)
Fe³+ (aq) + e
Ag (aq) + e
Ag(s)
Hg2+ (aq) + 2e
2Hg²+ (aq) + 2e →
NO3(aq) + 4H+ (aq) + 3e
2Hg(1)
40H (aq)
H₂O₂(aq) + 2H+ (aq) + 2e¯
Co³+ (aq) + e
O3(g) + 2H+ (aq) + 2e
F₂(g) + 2e →→→ 2F (aq)
Hg2+ (aq)
MnO₂ (s) + 4OH(aq)
H,Oz(aq)
Br₂(l) + 2e →→→ 2Br (aq)
O₂(g) + 4H+ (aq) + 4e¯
MnO₂ (s) + 4H+ (aq) + 2e →
Cr₂O² (aq) + 14H+ (aq) + 6e
Cl₂(g) + 2e →
Au³+ (aq) + 3e
2C1 (aq)
-
Au(s)
MnO4 (aq) + 8H+ (aq) + Se¯→→→→→
Ce+ (aq) + e
Ce ³+ (aq)
PbO₂ (s) + 4H+ (aq) + SO² (aq) + 2e¯
2H₂O
O₂(g) + H₂O(l)
NO(g) + 2H₂O
Co*(aq)
2H₂O
Mn²+ (aq) + 2H₂O
2Cr³+ (aq) + 7H₂O
2+
Mn²+ (aq) + 4H₂O
-> PbSO4(s) + 2H₂O
8° (V)
-3.05.
-2.93
-2.90
-2.89
-2.87
-2.71
-2.37
-1.85
-1.66
-1.18
-0.83
-0.76
-0.74
-0.44
-0.40
-0.31
-0.28
-0.25
-0.14
-0.13
0.00
+0.13
+0.15
+0.20
+0.22
+0.34
+0.40
+0.53
+0.59
+0.68
+0.77
+0.80
+0.85
+0.92
+0.96
+1.07
+1.23
+1.23
+1.33
+1.36
+1.50
+1.51
+1.61
+1.70
+1.77
+1.82
+2.07
+2.87
Increasing strength as reducing agent
*For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases.
These are the standard-state values.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6328ee4f-f12a-42a2-8e73-fa6d26b3c7cf%2F6d04a622-6cc5-456b-b212-e32460c54e39%2Fd1jdk1j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Table 20.1 Standard reduction potentials at 25°C*
Increasing strength as oxidizing agent
Half-Reaction
Li*(aq) + e
K+ (aq) + e
Ba²+ (aq) + 2e
Sr²+ (aq) + 2e-
Ca²+ (aq) + 2e
Na + (aq) + e
Mg²+ (aq) + 2e
Be²+ (aq) + 2e
Al³+ (aq) + 3e
Mn²+ (aq) + 2e
2H₂O + 2e™
Zn²+ (aq) + 2e-
Cr³+ (aq) + 3e
Fe²+ (aq) + 2e
Cd²+ (aq) + 2e
PbSO4(s) + 2e
Co²+ (aq) + 2e
Ni²+ (aq) + 2e
2+
Sn²+ (aq) + 2e
Pb²+ (aq) + 2e
Li(s)
K(s)
Ba(s)
→ Sr(s)
Ca(s)
Na(s)
Mg(s)
Be(s)
Al(s)
→→ Mn(s)
H₂(g) + 2OH(aq)
Zn(s)
Cr(s)
Fe(s)
Cd(s)
Pb(s) +
Co(s)
Ni(s)
Sn(s)
Pb(s)
H₂(g)
Sn²+ (aq)
+ SO² (aq)
4+
2H¹ (aq) + 2e
Sn¹+ (aq) + 2e
Cu²+ (aq) + e
→ Cut (aq)
SO (aq) + 4H+ (aq) + 2e SO₂(g) + 2H₂O
AgCl(s) + e → Ag(s) + Cl(aq)
Cu²+ (aq) + 2e
Cu(s)
O₂(g) + 2H₂O + 4e¯¯ →
[₂ (s) + 2e →→→→→→→ 21 (aq)
MnO4 (aq) + 2H₂O + 3e -
O₂(g) + 2H+ (aq) + 2e¯
Fe²+ (aq)
Fe³+ (aq) + e
Ag (aq) + e
Ag(s)
Hg2+ (aq) + 2e
2Hg²+ (aq) + 2e →
NO3(aq) + 4H+ (aq) + 3e
2Hg(1)
40H (aq)
H₂O₂(aq) + 2H+ (aq) + 2e¯
Co³+ (aq) + e
O3(g) + 2H+ (aq) + 2e
F₂(g) + 2e →→→ 2F (aq)
Hg2+ (aq)
MnO₂ (s) + 4OH(aq)
H,Oz(aq)
Br₂(l) + 2e →→→ 2Br (aq)
O₂(g) + 4H+ (aq) + 4e¯
MnO₂ (s) + 4H+ (aq) + 2e →
Cr₂O² (aq) + 14H+ (aq) + 6e
Cl₂(g) + 2e →
Au³+ (aq) + 3e
2C1 (aq)
-
Au(s)
MnO4 (aq) + 8H+ (aq) + Se¯→→→→→
Ce+ (aq) + e
Ce ³+ (aq)
PbO₂ (s) + 4H+ (aq) + SO² (aq) + 2e¯
2H₂O
O₂(g) + H₂O(l)
NO(g) + 2H₂O
Co*(aq)
2H₂O
Mn²+ (aq) + 2H₂O
2Cr³+ (aq) + 7H₂O
2+
Mn²+ (aq) + 4H₂O
-> PbSO4(s) + 2H₂O
8° (V)
-3.05.
-2.93
-2.90
-2.89
-2.87
-2.71
-2.37
-1.85
-1.66
-1.18
-0.83
-0.76
-0.74
-0.44
-0.40
-0.31
-0.28
-0.25
-0.14
-0.13
0.00
+0.13
+0.15
+0.20
+0.22
+0.34
+0.40
+0.53
+0.59
+0.68
+0.77
+0.80
+0.85
+0.92
+0.96
+1.07
+1.23
+1.23
+1.33
+1.36
+1.50
+1.51
+1.61
+1.70
+1.77
+1.82
+2.07
+2.87
Increasing strength as reducing agent
*For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases.
These are the standard-state values.
![1. Calculate AG and predict whether the following reaction would proceed spontaneously as
written at 298K:
2+
Mg(s) + Sn²+ (aq)
Mg²+ (aq) + Sn(s)
given that [Mg2+]=0.045 M, [Sn²+1=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6328ee4f-f12a-42a2-8e73-fa6d26b3c7cf%2F6d04a622-6cc5-456b-b212-e32460c54e39%2Fe9z3z9k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. Calculate AG and predict whether the following reaction would proceed spontaneously as
written at 298K:
2+
Mg(s) + Sn²+ (aq)
Mg²+ (aq) + Sn(s)
given that [Mg2+]=0.045 M, [Sn²+1=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)
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