Galvanic Cells
The energy released in a spontaneous
redox reaction can be used to perform electrical work. This occurs in a galvanic cell (aka a voltaic cell) which is a device in
which electron transfer is forced to take place through an external pathway,
rather than directly between reactants.
The two solid metals (Zn & Cu) are
called electrodes. The electrode at which oxidation occurs is
called the anode (Zn). The electrode at which reduction occurs is
called the cathode (Cu).
A voltaic cell consists of two half-reactions (reduction and
oxidation). Zn is oxidized at the anode to
produce electrons, which flow through the external
circuit to the cathode, where Cu2+ is reduced. Oxidation of Zn introduced extra Zn2+
ions into the anode compartment – unless this positive charge is neutralized,
no further oxidation can take place (also reduction of Cu2+ leaves
excess negative charge in the cathode compartment).
Electrical neutrality is maintained by
migration of ions through a salt bridge
(a glass U-tube filled with cotton batting soaked electrolyte solution - usually sodium nitrate).
The Na+ ions migrate to the cathode and the NO3-
ions migrate to the anode. The salt bridge also acts to close the circuit.
The
resulting electrochemical cell can
produce a voltage of 1.10 V
For the cell in which the reaction Zn°(s) + Cu2+(aq) →
Zn2+(aq) + Cu°(s) takes place, it can be written in a
short form, following the format below.
The │represents a phase boundary like that
between the electrode and the electrolyte.
The ║represents a physical boundary like the salt bridge.
anode(-) │electrolyte
║ electrolyte │cathode(+)
Zn(s)│Zn2+(aq)║
Cu2+(aq)│Cu(s)
TryIt!
For the Cu(s)│Cu2+(aq)║ Ag+(aq)│Ag(s) cell:
- Draw the cell, including beakers, specific electrodes, specific electrolytes, salt bridge , wires & voltmeter.
- Label the anode & cathode.
- Place the half cell reactions under the appropriate half cell.
- Show the direction of electron flow.
- Show the direction of ion flow.
- Write
out the net cell reaction.
Check out this video for the answer.
Cell Potential
So,
why do electrons flow spontaneously through the external circuit?
Like
all spontaneous processes, the answer involves energy. It is energetically favourable for electrons
to flow from the anode to the cathode of a voltaic cell, thus reducing their electrical potential energy. This is similar to the way in which it is energetically favourable for a boulder to roll down a hill to reduce its gravitational potential energy.
In
each half cell, the electrodes have different potential energies. In the above cell, the EP of the
electrons is higher in the Zn electrode than in the Cu electrode. If the electrodes are connected, the
electrons lower their EP by flowing from the Zn to the Cu electrode.
The
potential difference or voltage is measured in volts (V). The potential difference between the
electrodes of the cell is called the cell
potential (Ecell or E°) or cell voltage. The Zn/Cu cell
is 1.10 V at standard conditions (1.0 M solns and 1 atm gases, usually 25°C). So, 1.10 V is the standard cell potential (E°cell).
Standard Electrode Potentials
E°cell can be thought of as the sum of two half cell potentials (E°ox and E°red), the standard oxidation potential and the standard reduction potential:
E°cell = E°ox + E°red
We
can’t directly measure half cell potentials, so the standard reduction
potential of the
2H+(aq) + 2e- →
H2(g)
half-cell
has been assigned a value of 0 V and all other half cell potentials are measured
relative to this. This standard hydrogen electrode consists of
platinum wire to serve as an inert surface for the cathode reaction. The electrode is encased in a glass tube so H2(g)
can bubble over the platinum.
Still have questions? Check out this video.
Homework: #4-9 (found here)