Skip to main content
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 56b
Capitolo 20, Problema 56b

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.

Guida verificata passo dopo passo
1
Write the unbalanced chemical equation for the reaction: Cu^+ + NO_3^- -> Cu^{2+} + NO_2
Balance the chemical equation by ensuring the number of atoms and charges are equal on both sides. Consider the acidic solution, which allows you to add H^+ and H_2O as needed.
Use the standard reduction potentials from a table to find the half-reactions and their standard potentials. Calculate the standard emf (E°) for the reaction using E° = E°(cathode) - E°(anode).
Calculate the standard Gibbs free energy change (∆G°) using the formula ∆G° = -nFE°, where n is the number of moles of electrons transferred and F is the Faraday constant (96485 C/mol).
Calculate the equilibrium constant (K) at 298 K using the relationship ∆G° = -RTlnK, where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
10m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both the reactant and product sides. This is crucial for accurately representing the conservation of mass in a chemical reaction. In the context of the given reaction, it requires identifying the oxidation states of copper and nitrate ions and adjusting coefficients to achieve balance.
Video consigliato:
Percorso guidato
01:32
Balancing Chemical Equations

Standard Electrode Potential (emf)

The standard electrode potential (emf) is a measure of the tendency of a chemical species to be reduced, expressed in volts. It is determined under standard conditions (1 M concentration, 1 atm pressure, and 25°C). Calculating the standard emf for the reaction involves using standard reduction potentials from tables and applying the Nernst equation to find the overall cell potential.
Video consigliato:
Percorso guidato
01:27
Standard Cell Potential

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.
Video consigliato:
Percorso guidato
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. (a) Aqueous iodide ion is oxidized to I21s2 by Hg22+1aq2.

623
views
1
rank
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. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

312
views
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

(b) Calculate ∆G° for each reaction at 298 K.

369
views
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.

1
views
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

413
views