Questions: For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. - 2 Fe(s) + 3 Pb(NO3)2(aq) → 3 Pb(s) + 2 Fe(NO3)3(aq) - reactants oxidized: - reactants reduced: - Ca(s) + ZnCl2(aq) → Zn(s) + CaCl2(aq) - reactants oxidized: - reactants reduced: - Fel2(aq) + Mg(s) → Mgl2(aq) + Fe(s) - reactants oxidized: - reactants reduced:

For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. - 2 Fe(s) + 3 Pb(NO3)2(aq) → 3 Pb(s) + 2 Fe(NO3)3(aq) - reactants oxidized: - reactants reduced: - Ca(s) + ZnCl2(aq) → Zn(s) + CaCl2(aq) - reactants oxidized: - reactants reduced: - Fel2(aq) + Mg(s) → Mgl2(aq) + Fe(s) - reactants oxidized: - reactants reduced:
Transcript text: For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. \begin{tabular}{|c|c|} \hline \multirow{2}{*}{$2 \mathrm{Fe}(s)+3 \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \rightarrow 3 \mathrm{~Pb}(s)+2 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)$} & \begin{tabular}{l} reactants \\ oxidized: \end{tabular} \\ \hline & \begin{tabular}{l} reactants \\ reduced: \end{tabular} \\ \hline \multirow{2}{*}{$\mathrm{Ca}(s)+\mathrm{ZnCl}_{2}(a q) \rightarrow \mathrm{Zn}(s)+\mathrm{CaCl}_{2}(a q)$} & \begin{tabular}{l} reactants \\ oxidized: \end{tabular} \\ \hline & \begin{tabular}{l} reactants \\ reduced: \end{tabular} \\ \hline \multirow{2}{*}{$\mathrm{Fel}_{2}(a q)+\mathrm{Mg}(s) \rightarrow \mathrm{Mgl}_{2}(a q)+\mathrm{Fe}(s)$} & \begin{tabular}{l} reactants \\ oxidized: \end{tabular} \\ \hline & \begin{tabular}{l} reactants \\ reduced: \end{tabular} \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Identify Oxidation and Reduction in Reaction 1

For the reaction: \[ 2 \mathrm{Fe}(s) + 3 \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(aq) \rightarrow 3 \mathrm{Pb}(s) + 2 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(aq) \]

  • Oxidation: Iron (\(\mathrm{Fe}\)) is oxidized as it goes from \(\mathrm{Fe}(s)\) to \(\mathrm{Fe}^{3+}\) in \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\).
  • Reduction: Lead (\(\mathrm{Pb}^{2+}\)) is reduced as it goes from \(\mathrm{Pb}^{2+}\) in \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) to \(\mathrm{Pb}(s)\).
Step 2: Identify Oxidation and Reduction in Reaction 2

For the reaction: \[ \mathrm{Ca}(s) + \mathrm{ZnCl}_{2}(aq) \rightarrow \mathrm{Zn}(s) + \mathrm{CaCl}_{2}(aq) \]

  • Oxidation: Calcium (\(\mathrm{Ca}\)) is oxidized as it goes from \(\mathrm{Ca}(s)\) to \(\mathrm{Ca}^{2+}\) in \(\mathrm{CaCl}_{2}\).
  • Reduction: Zinc (\(\mathrm{Zn}^{2+}\)) is reduced as it goes from \(\mathrm{Zn}^{2+}\) in \(\mathrm{ZnCl}_{2}\) to \(\mathrm{Zn}(s)\).
Step 3: Identify Oxidation and Reduction in Reaction 3

For the reaction: \[ \mathrm{FeI}_{2}(aq) + \mathrm{Mg}(s) \rightarrow \mathrm{MgI}_{2}(aq) + \mathrm{Fe}(s) \]

  • Oxidation: Magnesium (\(\mathrm{Mg}\)) is oxidized as it goes from \(\mathrm{Mg}(s)\) to \(\mathrm{Mg}^{2+}\) in \(\mathrm{MgI}_{2}\).
  • Reduction: Iron (\(\mathrm{Fe}^{2+}\)) is reduced as it goes from \(\mathrm{Fe}^{2+}\) in \(\mathrm{FeI}_{2}\) to \(\mathrm{Fe}(s)\).

Final Answer

  1. Reaction 1:

    • Oxidized: \(\boxed{\mathrm{Fe}}\)
    • Reduced: \(\boxed{\mathrm{Pb}^{2+}}\)

  2. Reaction 2:

    • Oxidized: \(\boxed{\mathrm{Ca}}\)
    • Reduced: \(\boxed{\mathrm{Zn}^{2+}}\)

  3. Reaction 3:

    • Oxidized: \(\boxed{\mathrm{Mg}}\)
    • Reduced: \(\boxed{\mathrm{Fe}^{2+}}\)
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