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11 Dec 2019

From the standard reduction potentials in Table 11.1 in the Appendix, calculate the standard cell potential and the equilibrium constant at 298.15 K for the following reactions:

(a) 4 NiOOH(s) + 2 H2O(l) â 4 Ni(OH)2(s) + O2(g)

(b) 4 NO3 - (aq) + 4 H+ (aq) â 4 NO(g) + 2 H2O (l) + 3 O2(g)

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Collen VonLv2

13 Dec 2019

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Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at 298 K:

Fe(s) + Ni²⁺(aq)→ Fe²⁺(aq) + Ni(s)
Co(s) + 2 H⁺(aq)→Co²⁺(aq) + H₂(g)
10 Br^-(aq) + 2 MnO₄^-(aq) + 16 H⁺(aq)→ 2 Mn²⁺(aq) + 8 H₂O(aq) + 5 Br₂(l)

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Compare table 1 (the standard reduction potentials) to the periodic trends (radius, Ionization energy, electron affinity, electronegativity). Do the potentials in the table agree with our periodic trends? Why/why not (use at least two examples in your argument)?

Table 1: Standard Reduction Potentials
Half-Reaction	EÂ°, volts
Na⁺(aq) + e^â â Na(s)	-2.71
Al³⁺(aq) + 3 e^â â Al(s)	-1.66
Zn²⁺(aq) + 2 e^â â Zn(s)	-0.76
Cr³⁺(aq) + 3 e^â â Cr(s)	-0.74
Fe²⁺(aq) + 2 e^â â Fe(s)	-0.41
PbSO₄(s) + 2 e^â â Pb(s) + SO₄^2â(aq)	-0.36
Ni²⁺(aq) + 2 e^â â Ni(s)	-0.23
Sn²⁺(aq) + 2 e^â â Sn(s)	-0.14
Pb²⁺(aq) + 2 e^â â Pb(s)	-0.13
2 H⁺(aq) + 2 e^â â H₂(g)	0
Sn⁴⁺(aq) + 2 e^â â Sn²⁺(aq)	0.15
AgCl(s) + e^â â Ag(s) + Cl^â(aq)	0.22
Cu²⁺(aq) + 2 e^â â Cu(s)	0.34
O₂(g) + 2 H₂O(l) + 4 e^â â 4 OH^â(aq)	0.4
H₂SO₃(aq) + 4 H⁺(aq) + 4 e^â â S(s) + 3H₂O(l)	0.45
Ag⁺(aq) + e^â â Ag(s)	0.8
O₂(g) + 4 H⁺(aq) + 4 e^â â 2 H₂O(l)	1.23

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at 298 K:

(a) Cu(s) + 2 Ag⁺(aq)→Cu²⁺(aq) + 2 Ag(s)

(b) 3 Ce⁴⁺(aq) + Bi(s) + H₂O(l)→3Ce³⁺(aq) +BiO⁺(aq) + 2H⁺(aq)

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From the standard reduction potentials in Table 11.1 in the Appendix, calculate the standard cell potential and the equilibrium constant at 298.15 K for the following reactions:

(a) 4 NiOOH(s) + 2 H2O(l) â 4 Ni(OH)2(s) + O2(g)

(b) 4 NO3 - (aq) + 4 H+ (aq) â 4 NO(g) + 2 H2O (l) + 3 O2(g)

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From the standard reduction potentials in Table 11.1 in the Appendix, calculate the standard cell potential and the equilibrium constant at 298.15 K for the following reactions: (a) 4 NiOOH(s) + 2 H2O(l) â 4 Ni(OH)2(s) + O2(g) (b) 4 NO3 - (aq) + 4 H+ (aq) â 4 NO(g) + 2 H2O (l) + 3 O2(g)

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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From the standard reduction potentials in Table 11.1 in the Appendix, calculate the standard cell potential and the equilibrium constant at 298.15 K for the following reactions:

(a) 4 NiOOH(s) + 2 H2O(l) â 4 Ni(OH)2(s) + O2(g)

(b) 4 NO3 - (aq) + 4 H+ (aq) â 4 NO(g) + 2 H2O (l) + 3 O2(g)