Question

A voltaic cell that uses the reaction PdCl2−4(aq)+Cd(s)→Pd(s)+4Cl−(aq)+Cd2+(aq) has a measured standard cell potential of +1.03 V.

Part A) Write the two half-cell reactions. Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

Answer : The balanced two-half reactions will be,

Oxidation half reaction :
`Cd(s)\rightarrow Cd^(2+)(aq)+2e^-`

Reduction half reaction :
`Pd^(2+)(aq)+2e^-\rightarrow Pd(s)`

Explanation :

Voltaic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy. It is also known as the galvanic cell or electrochemical cell.

In the voltaic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

The given redox reaction is:

`PdCl_4^(2-)(aq)+Cd(s)\rightarrow Pd(s)+4Cl^-(aq)+Cd^(2+)(aq)`

The balanced two-half reactions will be,

Oxidation half reaction :
`Cd(s)\rightarrow Cd^(2+)(aq)+2e^-`

Reduction half reaction :
`Pd^(2+)(aq)+2e^-\rightarrow Pd(s)`