Electrochemistry 1 Flashcards
Electrochemistry
Electrochemistry is the study of production of
electricity from energy released during spontaneous
chemical reactions and the use of electrical energy
to bring about non-spontaneous chemical
transformations
. Batteries and fuel cells convert
Batteries and fuel cells
convert chemical energy into electrical energy and are
used on a large scale in various instruments and
devices.
galvanic or a
voltaic cell.
. This cell converts the chemical energy liberated during the
redox reaction to electrical energy and has an electrical
potential equal to 1.1 V when concentration
of Zn2+ and Cu2+ ions is unity (1 mol dm–3)*.
Zn(s) + Cu2+(aq) –> Zn2+(aq) + Cu(s)
electrolytic cell,
, a device for using
electrical energy to carry non-spontaneous
chemical reactions.
a situation where salt bridge is not required
Sometimes, both
the electrodes dip in the same electrolyte solution and in such cases we
do not require a salt bridge.
electrode potential.
A potential difference
develops between the electrode and the electrolyte which is called
electrode potential.
standard
electrode potential.
When the concentrations of all the species involved
in a half-cell is unity then the electrode potential is known as standard
electrode potential.
anode in galvanic cell
In a
galvanic cell, the half-cell in which oxidation takes place is called anode
and it has a negative potential with respect to the solution.
cathode in galvanic cell
The other
half-cell in which reduction takes place is called cathode and it has a
positive potential with respect to the solution.
cell potential
aka emf
The potential difference between the two electrodes of a galvanic
cell is called the cell potential and is measured in volts. The cell
potential is the difference between the electrode potentials (reduction
potentials) of the cathode and anode. It is called the cell electromotive
force (emf) of the cell when no current is drawn through the cell.
