Questions: In the reaction Zn + H^+ -> Zn^2+ + H2, Zn is oxidized and H is reduced. How many electrons would be produced and used in the balanced half-reactions? Complete the balanced half-reactions: H^+ + e^- -> H2 Zn -> Zn^2+ + e^-

In the reaction Zn + H^+ -> Zn^2+ + H2, Zn is oxidized and H is reduced.
How many electrons would be produced and used in the balanced half-reactions?

Complete the balanced half-reactions:

H^+ + e^- -> H2

Zn -> Zn^2+ + e^-

Transcript text: In the reaction $\mathrm{Zn}+\mathrm{H}^{+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{H}_{2}, \mathrm{Zn}$ is oxidized and H is reduced. How many electrons would be produced and used in the balanced half-reactions? Complete the balanced half-reactions: $\mathrm{H}^{+}+\square \mathrm{e}^{-} \rightarrow \square \mathrm{H}_{2}$ $\mathrm{Zn} \rightarrow$ $\square$ $\mathrm{Zn}^{2+}+$ $\mathrm{e}^{-}$

Solution

Solution Steps

Step 1: Identify the Oxidation and Reduction Half-Reactions

In the given reaction, zinc (Zn) is oxidized and hydrogen ions ($\mathrm{H}^+$) are reduced. We need to write the half-reactions for both processes.

Step 2: Write the Oxidation Half-Reaction

Zinc ($\mathrm{Zn}$) is oxidized to zinc ions ($\mathrm{Zn}^{2+}$). The oxidation half-reaction is: \[ \mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2\mathrm{e}^- \]

Step 3: Write the Reduction Half-Reaction

Hydrogen ions ($\mathrm{H}^+$) are reduced to hydrogen gas ($\mathrm{H}_2$). The reduction half-reaction is: \[ 2\mathrm{H}^+ + 2\mathrm{e}^- \rightarrow \mathrm{H}_2 \]

Step 4: Balance the Electrons in the Half-Reactions

Both half-reactions involve the transfer of 2 electrons. Therefore, they are already balanced in terms of electron transfer.

Final Answer

The balanced half-reactions are: \[ \boxed{2\mathrm{H}^+ + 2\mathrm{e}^- \rightarrow \mathrm{H}_2} \] \[ \boxed{\mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2\mathrm{e}^-} \]

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