Question

The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. type the half-cell reaction that takes place at the anode for the iron-silver voltaic cell. indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. use (aq) for an aqueous solution. do not include phases for electrons. express your answer as a chemical equation.

Answer 1

Answer:

$\boxed{\rm \text{Fe(s) \rightleftharpoons Fe ^{2+} (aq) + 2e ^{-} }}$

Explanation:

The half-cell reduction potentials are

Ag⁺(aq) +   e⁻ ⇌ Ag(s)     E° =  0.7996 V

Fe²⁺(aq) + 2e⁻ ⇌ Fe(s)     E° = -0.447    V

To create a spontaneous voltaic cell, we reverse the half-reaction with the more negative half-cell potential.

The anode is the electrode at which oxidation occurs.

The equation for the oxidation half-reaction is

$\boxed{\rm \textbf{Fe(s) \rightleftharpoons Fe ^{2+} (aq) + 2e ^{-} }}$

Answer 2

A voltaic cell is a type of cell in which energy is produced by redox reaction.

Voltaic cells are those cells that produce energy by means of a redox reaction. Hence, in a voltaic cell, chemical energy is converted to electrical energy.

The two half cells in this reaction  are the oxidation half cell and the reduction half cell.

For the oxidation half cell;

Fe(s) -------> Fe^2+(aq) + 2e

For the reduction half equation;

2Ag^+(aq) + 2e --------> 2Ag(s)

Note that the iron half cell is the anode while the silver half cell is the cathode.

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