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

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 serves as the 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 with hydrogen acting as the reducing agent.

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

These reactions are interconnected through the transfer of electrons, showcasing the principles of oxidation and reduction in electrochemistry. If you have any specific questions or need further analysis on any of these reactions, feel free to ask!
These reactions show how different metals and hydrogen interact, changing their oxidation states.

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

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