Ch.20 - Electrochemistry

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.20 - Electrochemistry

Problema 52c

Capitolo 20, Problema 52c

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

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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01:04

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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01:10

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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01:51

Gibbs Free Energy of Reactions

Pratica correlata

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

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

(a) Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s)

(b) Co(s) + 2 H⁺(aq) → Co²⁺(aq) + H₂(g)

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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

S₂O₆^2-(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

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