Voltaic Cells (DP IB Chemistry: HL)

• Voltaic (or Galvanic) cells generate electricity from spontaneous redox reactions
• For example:

Zn (s)  + CuSO₄ (aq)→ Cu (s)  + ZnSO₄ (aq)

• Instead of electrons being transferred directly from the zinc to the copper ions a cell is built which separates the two redox processes
• Each part of the cell is called a half cell
• If a rod of metal is dipped into a solution of its own ions, an equilibrium is set up
• For example:

Zn (s)  ⇌  Zn²⁺ (aq) + 2e^- 

When a metal is dipped into a solution contains its ions an equilibrium is established between the metal and it ions

• This is a half cell and the strip of metal is an electrode
• The position of the equilibrium determines the potential difference between the metal strip and the solution of metal
• The Zn atoms on the rod can deposit two electrons on the rod and move into solution as Zn²⁺ ions:

                   Zn(s) ⇌ Zn²⁺(aq) + 2e^- 

• This process would result in an accumulation of negative charge on the zinc rod
• Alternatively, the Zn²⁺ ions in solution could accept two electrons from the rod and move onto the rod to become Zn atoms:

                    Zn²⁺(aq) + 2e^-  ⇌ Zn(s)

• This process would result in an accumulation of positive charge on the zinc rod
• In both cases, a potential difference is set up between the rod and the solution
• This is known as an electrode potential

• A similar electrode potential is set up if a copper rod is immersed in a solution containing copper ions (eg CuSO₄), due to the following processes:

Cu²⁺(aq) + 2e^-  ⇌ Cu(s)   - reduction (rod becomes positive)

Cu(s) ⇌ Cu²⁺(aq) + 2e^-    - oxidation (rod becomes negative)

• Note that a chemical reaction is not taking place - there is simply a potential difference between the rod and the solution
• The potential difference will depend on
  • the nature of the ions in solution
  • the concentration of the ions in solution
  • the type of electrode used
  • the temperature

Creating an emf

• If two different electrodes are connected, the potential difference between the two electrodes will cause a current to flow between them. Thus an electromotive force (emf) is established and the system can generate electrical energy
• A typical electrochemical cell can be made by combining a zinc electrode in a solution of zinc sulphate with a copper electrode in a solution of copper sulphate

The zinc-copper voltaic cell ( also known as the Daniell Cell)

• The circuit must be completed by allowing ions to flow from one solution to the other
• This is achieved by means of a salt bridge - often a piece of filter paper saturated with a solution of an inert electrolyte such as KNO₃(aq)
• The e.m.f can be measured using a voltmeter
• Voltmeters have a high resistance so that they do not divert much current from the main circuit
• The combination of two electrodes in this way is known as an electrochemical or voltaic cell, and can be used to generate electricity

• The positive electrode or cathode is the one which most favours reduction
  • In this case it is the copper electrode which is positive

• The negative electrode or anode is the one which most favours oxidation
  • In this case it is the zinc electrode which is negative
• Thus electrons flow from the zinc electrode to the copper electrode

Ionic equations for the Daniell Cell

• To maintain charge in the half cells:
  • anions flow to the negative half cell to replace the negative charge of the electrons
  • cations flow to the positive half cell since there is a surplus positive charge from the metals becoming cations in the negative half cell
• The sulphate ions flow through the salt bridge from the Cu²⁺(aq) solution to the Zn²⁺(aq) solution, to complete the circuit and compensate for the reduced Cu²⁺ concentration and increased Zn²⁺ concentration
• The overall cell reaction including spectator ions can thus be written as follows:

Zn (s)  + CuSO₄ (aq)→ Cu (s)  + ZnSO₄ (aq)

• The external connection must be made of a metallic wire in order to allow electrons to flow
• The salt bridge must be made of an aqueous electrolyte to allow ions to flow
• By allowing two chemical reagents to be connected electrically, but not chemically, a reaction can only take place if the electrons flow externally
• The chemical energy is thus converted into electrical energy.