Calculate the standard cell potential for each of the electrochemical cells in Problem 44.

Verified step by step guidance

Identify the half-reactions involved in the electrochemical cell from Problem 44.

Write the reduction half-reaction and its standard reduction potential, E° (from a standard reduction potential table).

Write the oxidation half-reaction and its standard reduction potential, E° (from a standard reduction potential table).

Calculate the standard cell potential, E°_cell, using the formula: E°_cell = E°_cathode - E°_anode.

Ensure that the units are consistent and the final E°_cell is expressed in volts (V).

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Standard Cell Potential

The standard cell potential, denoted as E°, is the measure of the voltage produced by an electrochemical cell under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It indicates the tendency of a chemical reaction to occur spontaneously; a positive E° value suggests a spontaneous reaction, while a negative value indicates non-spontaneity.

Nernst Equation

The Nernst equation relates the cell potential to the concentrations of the reactants and products in an electrochemical reaction. It allows for the calculation of the cell potential under non-standard conditions, showing how changes in concentration affect the voltage. The equation is given by E = E° - (RT/nF)ln(Q), where Q is the reaction quotient.

Electrochemical Cells

Electrochemical cells consist of two half-cells, each containing an electrode and an electrolyte. The oxidation and reduction reactions occur at the anode and cathode, respectively. Understanding the components and functions of these cells is crucial for calculating the standard cell potential, as it involves identifying the correct half-reactions and their standard potentials.