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Oxidation Reduction ReactionsOxidation Reduction Reactions• (1) Oxidation: Loss e- Increase in Oxidation Number Zn(s) Zn2+ + 2e-
• (2) Reduction: Acceptance of e-
Decrease in Oxidation Number Cl2(g) + 2e- 2Cl-
• (1) Oxidation: Loss e- Increase in Oxidation Number Zn(s) Zn2+ + 2e-
• (2) Reduction: Acceptance of e-
Decrease in Oxidation Number Cl2(g) + 2e- 2Cl-
Balancing Oxidation-Reduction Equations:Balancing Oxidation-Reduction Equations: Use Half-Reaction MethodUse Half-Reaction Method
The half-reactions forSn2+(aq) + 2Fe3+(aq) Sn4+(aq) + 2Fe3+(aq)
areSn2+(aq) Sn4+(aq) +2e-
2Fe3+(aq) + 2e- 2Fe2+(aq)
• Oxidation Half-Reaction: electrons are products.
• Reduction Half-Reaction: electrons are reactants.
Half-Reaction Method for Balancing Half-Reaction Method for Balancing Oxidation-Reduction EquationsOxidation-Reduction Equations
1. Separate the equation into the two half-reactions. Write down the two half reactions.
2. Balance each half reaction:a. First balance all elements other than H and O.b. Then balance O by adding water.c. Then balance H by adding H+ if have acidic
solution.d. Finish by balancing charge by adding electrons.
3. Multiply each half reaction to make the number of electrons equal.
4. Add the two half-reactions and simplify. To simplify, remove components common to both reactant and product sides.
5. Check!
Example
Balance: (acidic)MnO4
- (aq) + Fe2+
(aq) Mn2+ (aq) + Fe3+
(aq)
1. The two incomplete half reactions areMnO4
-(aq) Mn2+(aq)
Fe2+ (aq) Fe3+
(aq)
8H+ + MnO4- + 5e- Mn2+ + 4 H2O
5 (Fe2+ (aq) Fe3+ (aq) + e-)
8H+ + MnO4- + 5 Fe2+ (aq) Mn2+ + 4 H2O + 5Fe3+ (aq)
Example
Balance: (basic)MnO4
- (aq) + I- (aq) MnO2
+ I2
1. The two incomplete half reactions areMnO4
-(aq) MnO2
I- (aq) I2
2 (2H2O + MnO4-(aq) + 3e- MnO2 + 4OH-)
3 (2I- (aq) I2 + 2e-)
4H2O + 6I- (aq) + MnO4-(aq) 2MnO2 + 8OH- + 3I2
Problem
Complete and balance the following equations, and identify the oxidizing and reducing agents
Cr2O72- (aq) + I-(aq) Cr3+(aq) + IO3-(aq)(acidic solution)
Pb(OH)42- (aq) + ClO- (aq) PbO2(s) + Cl-(aq)(basic solution)
How many moles of Cu can be plated out of a solution containing Cu2+ ions if a 1.50 amp current is passed through for 300 s?
Cu2+ + 2e- → Cu(s)
Notes: 1 amp = C/s F = 9.65 x 104 c/ mole e-
Find: c → moles e-s → moles Cu
= moles Cu1.50 c
s
300 s mole e-
9.65 x 104 C
1 mole Cu
2 mole e-s
2.33 x 10-3
Effect of Concentration on EMF
A Battery going dead.
∆G = ∆Go + RT lnQ
-nFE = -nFEo + RT ln Q
Dividing by –nF gives Rise to the Nerst Equation.
The Nerst Equation:
QlognF
2.303RT - E E :log 10 basefor Or o
logQn
0.0592 - E E : K 298 @ o
QlnnF
RT - E E o
Q: aA + bB ↔ cC + dD
ba
d
BA
D
][][
][[C] Q
c
mol K
J 314.8
R
molV
JxF
41065.9
n = # of e- s transferred
The Nerst Equation allows us to find voltage under nonstandard conditions
Example:
Determine E (voltage) for: Fe(s) + Cd2+(aq) → Fe2+
(aq) + Cd(s)
When [Fe2+] = 0.10 M and [Cd2+] = 1.0 M @ 298K
Half RXNs: Fe(s) → Fe2+ + 2e- Eo = +0.44 V
Cd2+ + 2e- → Cd(s) Eo = -0.40 V
Eo = +0.04 V
][
][log
0592.02
2
Cd
Fe
nEE o
VVE 07.0]0.1[
]10.0[log
2
0592.004.0 + Value means spontaneous
Now try: [Fe2+] = 1.0 M and [Cd2+] = 0.01 M @ 298K
VVE 02.0]01.0[
]0.1[log
2
0592.004.0
- Value means non spontaneous and will go in opposite direction
What does an E = 0 value mean?
logQn
0.0592 - E E : K 298 @ o
logKn
0.0592 - E 0 E : K 298 @ o
0.0592
nElogK : K 298 @
o
For: Fe(s) + Cd2+(aq) → Fe2+(aq) + Cd(s) Eo = +0.04V
35.10.0592
0.04V))(e (2mollogK : K 298 @
-
K = 22