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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.20 - ElectrochemistryProblema 118
Capitolo 20, Problema 118

The Ksp value for PbS(s) is 8.0 * 10^-28. By using this value together with an electrode potential from Appendix E, determine the value of the standard reduction potential for the reaction PbS(s) + 2 e^- → Pb(s) + S^2-(aq).

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Identify the dissolution reaction for PbS(s) in water: PbS(s) ⇌ Pb^{2+}(aq) + S^{2-}(aq). The solubility product constant (K_{sp}) is given for this reaction.
Write the Nernst equation for the half-reaction: PbS(s) + 2 e^- → Pb(s) + S^{2-}(aq). This involves the standard reduction potential (E°) and the reaction quotient (Q).
Use the relationship between the Gibbs free energy change (ΔG°) and the equilibrium constant (K_{sp}): ΔG° = -RT ln(K_{sp}). Calculate ΔG° using the given K_{sp} value.
Relate ΔG° to the standard reduction potential (E°) using the equation: ΔG° = -nFE°, where n is the number of moles of electrons transferred (n=2 for this reaction) and F is the Faraday constant.
Solve for the standard reduction potential (E°) using the calculated ΔG° and the relationship ΔG° = -nFE°.

Concetti chiave

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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It represents the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced equation. For PbS, Ksp = [Pb^2+][S^2-], and a low Ksp value indicates that the compound is not very soluble in water.
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Solubility Product Constant

Electrode Potential

Electrode potential is a measure of the tendency of a chemical species to be reduced, expressed in volts. It is determined under standard conditions and is crucial for predicting the direction of redox reactions. The standard reduction potential for a half-reaction can be found in tables, and it helps in calculating the overall cell potential when combined with other half-reactions.
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Standard Cell Potential

Nernst Equation

The Nernst equation relates the reduction potential of a half-cell to the concentrations of the reactants and products involved in the reaction. It allows for the calculation of the cell potential under non-standard conditions. This equation is essential for determining how changes in concentration affect the electrode potential, which is necessary for solving the given problem involving PbS.
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The Nernst Equation
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Cytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe to supply energy required to synthesize adenosine triphosphate (ATP). The body uses ATP as an energy source to drive other reactions (Section 19.7). At pH 7.0 the following reduction potentials pertain to this oxidation of CyFe2+: O21g2 + 4 H+1aq2 + 4 e- ¡ 2 H2O1l2 Ered ° = +0.82 V CyFe3+1aq2 + e- ¡ CyFe2+1aq2 E°red = +0.22 V (a) What is ∆G for the oxidation of CyFe2+ by air? (b) If the synthesis of 1.00 mol of ATP from adenosine diphosphate (ADP) requires a ∆G of 37.7 kJ, how many moles of ATP are synthesized per mole of O2?

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A student designs an ammeter (a device that measures electrical current) that is based on the electrolysis of water into hydrogen and oxygen gases. When electrical current of unknown magnitude is run through the device for 2.00 min, 12.3 mL of water-saturated H21g2 is collected. The temperature of the system is 25.5 °C, and the atmospheric pressure is 768 torr. What is the magnitude of the current in amperes?

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Domanda del libro di testo

Cytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe to supply energy required to synthesize adenosine triphosphate (ATP). The body uses ATP as an energy source to drive other reactions (Section 19.7). At pH 7.0 the following reduction potentials pertain to this oxidation of CyFe2+: O21g2 + 4 H+1aq2 + 4 e- ¡ 2 H2O1l2 Ered ° = +0.8 (b) If the synthesis of 1.00 mol of ATP from adenosine diphosphate (ADP) requires a ∆G of 37.7 kJ, how many moles of ATP are synthesized per mole of O2?

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