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chapter 18 - electrochem
18.2 galvanic cells
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galvanic cells are used for
spontaneous
reactions
a
reducing agent
causes other things to be
reduced
an oxidizing agent causes other things to be
oxidized
Zn(s) + Cu2+(aq) -> Zn2+ (aq) + Cu(s)
Zn
is
oxidized
Cu2+
is reduced
Zn
is the
reducing
agent
Cu2+
is the
oxidizing
agent
the
anode
is where oxidation occurs
the
cathode
is where reduction occurs
anode
II
cathode
single
line between phases
electrodes
first
and
last
cannot create a cell without a
solid metal electrode
difference in electrical potential between the anode and cathode is called the
cell voltage
hydrogen electrodes have a potential of
zero
the
standard
hydrogen electrode is used as
reference
point to measure other
voltages
E° = standard
reduction
potential =
voltage reduction rxn
at
standard conditions
voltage is
independent
of amount