1. A bar of zinc metal is immersed in a solution of copper (II) sulfate.
2. A strip of magnesium metal is placed in a solution of iron (II) chloride.

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Accepted Answer

***A*** ∻Key Concept∻ ⚹Single Displacement Reactions⚹ ∻Explanation∻ ⚹In a single displacement reaction, a more reactive metal displaces a less reactive metal from its compound. In the case of zinc and copper (II) sulfate, zinc is more reactive than copper and will displace copper from the sulfate to form zinc sulfate and copper metal. The reaction can be represented by the equation: $Zn(s) + CuSO_4(aq) \rightarrow ZnSO_4(aq) + Cu(s)$. Similarly, magnesium is more reactive than iron, so when magnesium is placed in iron (II) chloride solution, it will displace the iron to form magnesium chloride and iron metal, as shown by the equation: $Mg(s) + FeCl_2(aq) \rightarrow MgCl_2(aq) + Fe(s)$.⚹ ***B*** ∻Key Concept∻ ⚹Reactivity Series⚹ ∻Explanation∻ ⚹The reactivity series is a list of metals arranged in order of decreasing reactivity. Metals higher in the series will displace metals lower in the series from their compounds in solution. This concept explains why zinc can displace copper and magnesium can displace iron in the given reactions.⚹◊What are the chemical equations for the single displacement reactions described involving zinc metal and magnesium metal?⍭ Generate me a similar question◊

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