$$ \left. \begin{array} { l } { Cu ^ { 2 + } + Zn ightarrow Zn ^ { 2 + } + Cu } \ { 2 Al + 6 H ^ { + } ightarrow 2 AL ^ { 3 + } + 3 H _ { 2 } } \ { Cu ^ { 2 + } + H _ { 2 } ightarrow Cu + 2 H ^ { + } } \end{array} ight. $$

Question

$$ \left. \begin{array} { l } { Cu ^ { 2 + } + Zn ightarrow Zn ^ { 2 + } + Cu } \ { 2 Al + 6 H ^ { + } ightarrow 2 AL ^ { 3 + } + 3 H _ { 2 } } \ { Cu ^ { 2 + } + H _ { 2 } ightarrow Cu + 2 H ^ { + } } \end{array} ight. $$

UpStudy AI · Accepted Answer

Let's analyze the given chemical reactions step by step.

1. **First Reaction:**
   $$
   Cu^{2+} + Zn \rightarrow Zn^{2+} + Cu
   $$
   - In this reaction, copper ions ($$Cu^{2+}$$) are reduced to copper metal ($$Cu$$), while zinc metal ($$Zn$$) is oxidized to zinc ions ($$Zn^{2+}$$). This is a redox reaction where zinc acts as a reducing agent.

2. **Second Reaction:**
   $$
   2 Al + 6 H^{+} \rightarrow 2 Al^{3+} + 3 H_{2}
   $$
   - Here, aluminum ($$Al$$) is oxidized to aluminum ions ($$Al^{3+}$$), and hydrogen ions ($$H^{+}$$) are reduced to hydrogen gas ($$H_{2}$$). This is also a redox reaction where aluminum acts as a reducing agent.

3. **Third Reaction:**
   $$
   Cu^{2+} + H_{2} \rightarrow Cu + 2 H^{+}
   $$
   - In this reaction, copper ions ($$Cu^{2+}$$) are reduced to copper metal ($$Cu$$), while hydrogen gas ($$H_{2}$$) is oxidized to hydrogen ions ($$H^{+}$$). Again, this is a redox reaction where hydrogen acts as a reducing agent.

### Summary of Reactions:
- The first reaction shows the reduction of copper ions by zinc.
- The second reaction shows the oxidation of aluminum and the reduction of hydrogen ions.
- The third reaction shows the reduction of copper ions by hydrogen gas.

These reactions illustrate the principles of oxidation and reduction, where one species is oxidized (loses electrons) and another is reduced (gains electrons).
The reactions show how different elements are oxidized and reduced. In the first reaction, zinc reduces copper ions to copper metal. In the second, aluminum is oxidized to aluminum ions while hydrogen is reduced to hydrogen gas. The third reaction has copper ions reduced to copper metal by hydrogen gas.

\( \left. \begin{array} { l } { Cu ^ { 2 + } + Zn \rightarrow Zn ^ { 2 + } + Cu } \\ { 2 Al + 6 H ^ { + } \rightarrow 2 AL ^ { 3 + } + 3 H _ { 2 } } \\ { Cu ^ { 2 + } + H _ { 2 } \rightarrow Cu + 2 H ^ { + } } \end{array} \right. \)

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