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2. Direction of Oxidation-Reduction Reaction Strong oxidizing agent+ Strong reducing agent
→ Weak reducing agent + Weak oxidizing agent
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Solution:
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F (Faraday Constant常量 = 9.648531 × 104 C• mol-1 常量) 常量
Measuring:
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Example:
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Solution: (1)
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(2)
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三. Electrode Potential (Reduction Potential ) 电极电势（还原电势） 电极电势（还原电势）
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二.Electrochemistry Cell电化学电池 电化学电池
1. Construction of Voltaic (Galvanic) Cell原电池 原电池:
Chemical reactions to produce electricity
Cell
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11
i) Negative electrode (anode)负极（阴极）: 负极（ 负极 阴极） loss of electron, oxidation, reducing agent.
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Electrode Reaction:
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Nernst Equation:
34
35
Example:
When:
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Solution: 1)
Negative Electrode:
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Positive Electrode:
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B . Effect of Insoluble Compound or Complex on Electrode Potential
1
Electrochemistry电化学 电化学: 电化学 is the branch of chemistry that deals with the use of spontaneous chemical reactions to produce electricity and the use of electricity to bring about non-spontaneous chemical change. 研究自发化学反应产生电和电引起非自发化学变 化的化学分支学科
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Electrode reaction:
-)
Overall Cell Reaction:
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Example: T =298.15K:
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Solution:
Electrode reaction:
-)
Overall Cell Reaction:
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4. Potential Diagram of Element Oxidation Number: higher → lower
2. Balancing a redox equation : 配平氧化还原方程 a) Mass balance 质量守衡 b) Charge balance电荷守衡 Step步骤 步骤: 步骤 1) Reactants and products (ionic forms) 反应物和产物（离子形式 离子形式） 反应物和产物 离子形式） 2) Half reactions半反应 半反应 3)Balance half reaction配平半反应 配平半反应
1.Reference electrode:参考电极 参考电极
A) SHEB). SCE:甘汞电极 甘汞电极
EƏ = 0.2415V
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2. Standard Electrode Potential标准电极电势 标准电极电势
a) Negative electrode (anode)负极（阴极） : 负极（阴极） 负极
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Inert electrode惰性电极 Platinum铂, Graphite石墨 惰性电极: 铂 惰性电极 石墨
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i) Negative electrode (anode)负极（阴极）: 负极（ 负极 阴极）
ii) Positive electrode (cathode)正极（阳极）: 正极（ 正极 阳极）
4) Add after multiplication乘以最小公倍数后加 乘以最小公倍数后加
5) Check检查 检查
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I. Basic solution碱性溶液: MnO4- + Br - → 1) MnO4- + Br 2) 3) a. → MnO2 +BrO3-
7
b.
c.
d.
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e.
4.
5.
ii) Positive electrode (cathode)正极 正极: 正极 gain of electron, reduction, oxidizing agent.
iii) Salt bridge盐桥 KCl 盐桥: 盐桥 iv) External circuit (wire)外电路 外电路
Oxidized form +z e-
Reduced form
The more positive the reduction potential, the stronger the species on the left is as an oxidizing agent and the weaker the species on the right is as a reducing agent
(cathode)正极（阳 正极（ 正极 极）: reduction
Overall cell reaction:
总反应
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( 3):
a) Negative electrode 负极（ (anode)负极（阴极） : 负极 阴极）
oxidation b) Positive electrode
(cathode)正极（阳 正极（ 正极 极）: reduction
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Example:
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Acidic:
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A) Judging Disproportionate Reaction Example: Acidic: Solution:
-)
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Conclusion: ER Ə> E LƏ, Disproportionate reaction occurs B) Calculating Standard Electrode Potential
oxidation b) Positive electrode
(cathode)正极（阳 正极（ 正极 极）: reduction
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3. Nernst Equation: A: Nernst Equation
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F (Faraday Constant) = 9.648531 × 104 C• mol-1
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Solution: (1)
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(2)
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3. Extent of Oxidation-Reduction Reaction
T =298.15K
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Example:
Solution:
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Example: T= 298.15K
Solution: Design following cell
2
Importance
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一.Basic Concept: 1. Oxidation Number氧化数 : 氧化数
Cu(aq) + AgNO3 (aq) ↔ Cu (NO3)2 (aq) + Ag(s)
Oxidation-reduction (redox) reaction: transfer of electrons from species to another. Oxidation氧化 electron loss失去电子 氧化: 氧化 失去电子 Reduction: Electron gain得到电子 得到电子
Chapter 7 Oxidation- Reduction Reaction -Base of Electrochemistry 氧化-还原反应（电化学基础） 氧化 还原反应（电化学基础） 还原反应 Outline: 1.Basic Concept基本概念 Concept基本概念 2. Electrochemistry Cell电化学电池 电化学电池 3. Electrode Potential电极电势 电极电势 4. Application of Electrode Potential 电极电势的应用
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Solution: Oxidation/Reduction Pair
Equilibrium 1:
40
Equilibrium 2:
41
42
=
43
Example:
Solution:
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46
=
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四. Application of Electrode Potential
1. Relative Strengths of Oxidizing and Reducing Agents
Oxidizing agent (oxidant):氧化剂 氧化剂：eletron acceptor 氧化剂 (oxidized)电子受体（被氧化） 电子受体（ 电子受体 被氧化） Reducing agent ( reductant )还原剂: electron donor (reduced)电子给体（还原） 电子给体（还原）