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 72a
Capitolo 20, Problema 72a

A voltaic cell utilizes the following reaction: 2 Fe3+1aq2 + H21g2 ¡ 2 Fe2+1aq2 + 2 H+1aq2 (a) What is the emf of this cell under standard conditions?

Guida verificata passo dopo passo
1
Step 1: Identify the half-reactions involved in the overall cell reaction.
Step 2: Write the reduction half-reaction and the oxidation half-reaction separately.
Step 3: Use the standard reduction potentials from a table to find the potential for each half-reaction.
Step 4: Calculate the standard cell potential (emf) by subtracting the oxidation potential from the reduction potential.
Step 5: Ensure the units are consistent and the final expression is in volts (V).

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:
4m

Concetti chiave

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

Electrochemical Cells

Electrochemical cells are devices that convert chemical energy into electrical energy through redox reactions. A voltaic cell, specifically, generates electricity spontaneously from a chemical reaction, involving oxidation and reduction processes occurring in separate half-cells. Understanding the structure and function of these cells is essential for analyzing their emf (electromotive force) and overall efficiency.
Video consigliato:
Percorso guidato
02:46
Electrochemical Cells

Standard Electrode Potentials

Standard electrode potentials are measured voltages that indicate the tendency of a species to be reduced, measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C). Each half-reaction in a voltaic cell has a specific standard electrode potential, which can be used to calculate the overall cell potential (emf) by subtracting the anode potential from the cathode potential. This concept is crucial for determining the emf of the cell in the given reaction.
Video consigliato:
Percorso guidato
01:27
Standard Cell Potential

Nernst Equation

The Nernst equation relates the emf of an electrochemical cell to the concentrations of the reactants and products involved in the redox reaction. It allows for the calculation of the cell potential under non-standard conditions, taking into account temperature and concentration variations. Understanding this equation is important for predicting how the emf changes as the reaction progresses or as conditions vary.
Video consigliato:
Percorso guidato
01:17
The Nernst Equation
Pratica correlata
Domanda del libro di testo

A voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 (b) What is the emf of this cell when 3Fe2+4 = 1.3 M, 3Fe3+4= 0.010 M, PO2 = 0.50 atm, and the pH of the solution in the cathode half-cell is 3.50?

742
views
Domanda del libro di testo

A voltaic cell is constructed that is based on the following reaction: Sn2+(aq) + Pb(s) → Sn(s) + Pb2+(aq) (a) If the concentration of Sn2+ in the cathode half-cell is 1.00 M and the cell generates an emf of +0.22 V, what is the concentration of Pb2+ in the anode half-cell?

936
views
Domanda del libro di testo

A voltaic cell utilizes the following reaction: (b) What is the emf for this cell when 3Fe3+4 = 3.50 M, PH2= 0.95 atm, 3Fe2+4 = 0.0010 M, and the pH in both half-cells is 4.00?

1012
views
1
comments
Domanda del libro di testo

A voltaic cell utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 (a) What is the emf of this cell under standard conditions?

398
views