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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.20 - ElectrochemistryProblema 56c
Capitolo 20, Problema 56c

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

Guida verificata passo dopo passo
1
Step 1: Write the balanced redox reaction.
Step 2: Calculate the standard cell potential (E°cell) using standard reduction potentials.
Step 3: Use the Nernst equation to calculate the standard Gibbs free energy change (∆G°) at 298 K.
Step 4: Use the relationship between ∆G° and the equilibrium constant (K) to calculate K at 298 K.
Step 5: Verify the balanced equation and calculations for consistency and accuracy.

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Balancing Redox Reactions

Balancing redox reactions involves ensuring that the number of atoms and the charge are equal on both sides of the equation. This process often requires identifying the oxidation and reduction half-reactions, balancing them separately, and then combining them to form a complete balanced equation. In this case, understanding the oxidation states of chromium in Cr(OH)2 and CrO4^2- is essential.
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Balancing Basic Redox Reactions

Standard Electromotive Force (emf)

The standard electromotive force (emf) of a reaction is the voltage produced by an electrochemical cell under standard conditions. It can be calculated using the standard reduction potentials of the half-reactions involved. A positive emf indicates a spontaneous reaction, while a negative emf suggests non-spontaneity. This concept is crucial for determining the feasibility of the redox reaction in question.
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Standard Reduction Potentials

Gibbs Free Energy and Equilibrium Constant

Gibbs free energy (∆G°) is a thermodynamic quantity that indicates the spontaneity of a reaction at constant temperature and pressure. The relationship between ∆G° and the equilibrium constant (K) is given by the equation ∆G° = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin. This relationship allows for the calculation of K from ∆G° and vice versa, providing insight into the position of equilibrium for the reaction.
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Gibbs Free Energy of Reactions
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Domanda del libro di testo

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion.

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Domanda del libro di testo

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (a) Aqueous iodide ion is oxidized to I21s2 by Hg22+1aq2.

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Domanda del libro di testo

Given the following reduction half-reactions:

Fe3+(aq) + e- → Fe2+(aq) E°red = +0.77 V

S2O62-(aq) + 4 H+(aq) + 2 e- → 2 H2SO3(aq) E°red = +0.60 V

N2O(g) + 2 H+(aq) + 2 e- → N2(g) + H2O(l) E°red = -1.77 V

VO2+(aq) + 2 H+(aq) + e- → VO2+ + H2O(l) E°red = +1.00 V

(c) Calculate the equilibrium constant K for each reaction at 298 K.

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Domanda del libro di testo

From each of the following pairs of substances, use data in Appendix E to choose the one that is the stronger reducing agent: (d) BrO3-1aq2 or IO3-1aq2

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