Skip to main content
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 57a
Capitolo 20, Problema 57a

A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction
(a) if n = 1?

Guida verificata passo dopo passo
1
Identify the relationship between the standard cell potential (E°) and the equilibrium constant (K) using the Nernst equation at standard conditions.
Use the formula: E° = (RT/nF) * ln(K), where R is the universal gas constant (8.314 J/mol·K), T is the temperature in Kelvin (298 K), n is the number of moles of electrons transferred in the reaction, and F is Faraday's constant (96485 C/mol).
Rearrange the formula to solve for the equilibrium constant (K): ln(K) = (nF * E°) / (RT).
Substitute the given values into the equation: n = 1, E° = 0.177 V, R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol.
Calculate ln(K) using the substituted values, and then find K by taking the exponential of ln(K).

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:
7m

Concetti chiave

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

Standard Cell Potential

The standard cell potential (E°) is the measure of the voltage produced by an electrochemical cell under standard conditions (1 M concentration, 1 atm pressure, and 298 K). It indicates the tendency of a chemical reaction to occur spontaneously; a positive E° suggests a spontaneous reaction, while a negative E° indicates non-spontaneity.
Video consigliato:
Percorso guidato
01:27
Standard Cell Potential

Nernst Equation

The Nernst equation relates the cell potential to the concentrations of the reactants and products in an electrochemical reaction. It can be used to calculate the equilibrium constant (K) by connecting E° to the Gibbs free energy change (ΔG°) and the reaction quotient (Q), allowing for the determination of K at equilibrium.
Video consigliato:
Percorso guidato
01:17
The Nernst Equation

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is derived from the standard cell potential and reflects the extent to which a reaction proceeds; a larger K indicates a greater tendency for products to form, while a smaller K suggests a preference for reactants.
Video consigliato:
Percorso guidato
01:14
Equilibrium Constant K
Pratica correlata
Domanda del libro di testo

At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the reaction is 5.5 × 105. What is the value of n for the reaction?

103
views
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)

(c) 10 Br-(aq) + 2 MnO4-(aq) + 16 H+(aq) → 2 Mn2+(aq) + 8 H2O(l) + 5 Br2(l)

1162
views
Domanda del libro di testo

A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction (b) if n = 2? (c) if n = 3?

818
views
1
rank