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?

검증된 단계별 안내

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).

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주요 개념

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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.

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.

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.