REDOX PRACTICE MONDAY 4/07/08
1)
Balance the redox reaction given C0 C+4 and Fe+3  Fe0 react, answer the following:
a) Balance both half reactions.
a) What species is reduced.
b) What species is oxidized
c) How many moles of electrons are transferred in the oxidation?
C0  C+4 + 4e3e- + Fe+3  Fe0
C0  C+4 + 4e3e- + Fe+3  Fe0
Add electrons to most + side to balance
Balance the electrons by finding the LCD of 4
and 3 which is 12, THEN multiply each
reaction by the factor that gives 12 electrons.
3[C0  C+4 + 4e- ]
4[3e- + Fe+3  Fe0]
Balance the electrons by finding the LCD of 4
and 3 which is 12, THEN multiply each
reaction by the factor that gives 12 electrons.
12 mol of electrons
transferred
3C0  3C+4 + 12e- 0
C IS OXIDIZED AND LOSES ELECTRONS
12e- + 4Fe+3  4Fe0
4Fe+3 + 3C0  3C+4 + 4Fe0 Fe IS REDUCED AND GAINS ELECTRONS
+3