For each reaction in the data table, perform the following steps:Write the overall single-displacement reaction.Write the half-cell reaction for oxidation.Write the half-cell reaction for reduction.Add the two half-cell reactions, and write the net ionic equation.Identify the reducing agent.• Identify the oxidizing agent No. ofMetal Tested Mg2* (M9SO4)Fe2* (FeSOA)Cu2* (CUSOA)ReactionsBubblesBubblesformed, Mgstrip turnedbrowned and greenish andgrayish color.The solution isformed, MgpieceMg(s)Bubble formed7the FeS04solutiondarkenedwith the rustdarkenedwith rustCoppercoloroccurredBlackLight Rustformedon part ofpin thatFe(s)3coatingformedwasexposed tothe solutionNo reactionNo reactionNo reactionCu(s)OCcurredoCcurredOCcurred

According to reactivity series, Mg is most reactive and copper is least reactive metal amongst these three. Mg can displace Fe and Cu both. Fe can displace only copper. Cu cannot displace Fe and Cu. Oxidation reaction - loss of electrons / increase in oxidation number Reduction reaction- gain of electrons / decrease in oxidation number Oxidizing agent- reagent that itself undergo reduction Reducing agent- reagent that itself undergo oxidation1) Mg Write the overall single-displacement reaction. Mg (s) + FeSO4 (aq) → MgSO4 (aq) + Fe (s) Mg (s) + CuSO4 (aq) → MgSO4 (aq) + Cu (s) Write the half-cell reaction for oxidation. Mg (s) → Mg2+ (aq) + 2e Mg (s) → Mg2+ (aq) + 2e- Write the half-cell reaction for reduction. Fe2+ (aq) + 2e- → Fe (s) Cu2+ (aq) + 2e- → Cu (s) Add the two half-cell reactions, and write the net ionic equation. Mg (s) + Fe2+ (aq) → Mg2+ (aq) + Fe (s) Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s) Identify the reducing agent. Mg is reducing agent Mg is reducing agent Identify the oxidizing agent FeSO4 is oxidizing agent CuSO4 is oxidizing agent 2) Fe Write the overall single-displacement reaction. Fe (s) + CuSO4 (aq) → FeSO4 (aq) + Cu (s) Write the half-cell reaction for oxidation. Fe (s) → Fe2+ (aq) + 2e- Write the half-cell reaction for reduction. Cu2+ (aq) + 2e- → Cu (s) Add the two half-cell reactions, and write the net ionic equation. Fe (s) + Cu2+ (aq) → Fe2+ (aq) + Cu (s) Identify the reducing agent. Fe is reducing agent Identify the oxidizing agent CuSO4 is oxidizing agent