For each single-replacement reaction that proceeded spontaneously, write a set of redox half reactions and identify the oxidizing and reducing agents.

Cu and Ag 

Zn and cu 

Zn and ag

Mg and cu 

Mg and zn 

Mg and ag 




Let's break down each single-replacement reaction, write the corresponding redox half-reactions, and identify the oxidizing and reducing agents.

### 1. Cu and Ag

**Reaction:**
\[ \text{Cu} + \text{AgNO}_3 \rightarrow \text{Cu(NO}_3\text{)}_2 + \text{Ag} \]

**Oxidation Half-Reaction:**
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \]

**Oxidizing Agent:** \( \text{Ag}^+ \) (Silver ion)
**Reducing Agent:** \( \text{Cu} \) (Copper metal)

### 2. Zn and Cu

**Reaction:**
\[ \text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu} \]

**Oxidation Half-Reaction:**
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \]

**Oxidizing Agent:** \( \text{Cu}^{2+} \) (Copper ion)
**Reducing Agent:** \( \text{Zn} \) (Zinc metal)

### 3. Zn and Ag

**Reaction:**
\[ \text{Zn} + 2\text{AgNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + 2\text{Ag} \]

**Oxidation Half-Reaction:**
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ 2\text{Ag}^+ + 2e^- \rightarrow 2\text{Ag} \]

**Oxidizing Agent:** \( \text{Ag}^+ \) (Silver ion)
**Reducing Agent:** \( \text{Zn} \) (Zinc metal)

### 4. Mg and Cu

**Reaction:**
\[ \text{Mg} + \text{CuSO}_4 \rightarrow \text{MgSO}_4 + \text{Cu} \]

**Oxidation Half-Reaction:**
\[ \text{Mg} \rightarrow \text{Mg}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \]

**Oxidizing Agent:** \( \text{Cu}^{2+} \) (Copper ion)
**Reducing Agent:** \( \text{Mg} \) (Magnesium metal)

### 5. Mg and Zn

**Reaction:**
\[ \text{Mg} + \text{ZnSO}_4 \rightarrow \text{MgSO}_4 + \text{Zn} \]

**Oxidation Half-Reaction:**
\[ \text{Mg} \rightarrow \text{Mg}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \]

**Oxidizing Agent:** \( \text{Zn}^{2+} \) (Zinc ion)
**Reducing Agent:** \( \text{Mg} \) (Magnesium metal)

### 6. Mg and Ag

**Reaction:**
\[ \text{Mg} + 2\text{AgNO}_3 \rightarrow \text{Mg(NO}_3\text{)}_2 + 2\text{Ag} \]

**Oxidation Half-Reaction:**
\[ \text{Mg} \rightarrow \text{Mg}^{2+} + 2e^- \]

**Reduction Half-Reaction:**
\[ 2\text{Ag}^+ + 2e^- \rightarrow 2\text{Ag} \]

**Oxidizing Agent:** \( \text{Ag}^+ \) (Silver ion)
**Reducing Agent:** \( \text{Mg} \) (Magnesium metal)

Would you like further details or have any questions?

Here are five more questions you can ask:
1. What is the general rule for predicting single-replacement reactions?
2. How do you balance redox reactions in acidic solutions?
3. How do you balance redox reactions in basic solutions?
4. What are some common oxidizing and reducing agents?
5. Can you explain the activity series and its role in predicting reaction spontaneity?

**Tip:** In redox reactions, always identify which species gets oxidized (loses electrons) and which gets reduced (gains electrons) to determine the oxidizing and reducing agents.

Learn about single-replacement reactions, redox half-reactions, and how to identify oxidizing and reducing agents in reactions involving Cu, Ag, Zn, and Mg. Detailed explanations and examples provided.

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