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

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