Question

What are the products of a single-displacement reaction when magnesium metal (Mg) reacts with copper sulfate (CuS04)?

Answer 1

$\underline \bold{REACTIVITY \: SERIES}$

Its the series in which elements are arranged in the decreasing order of their reactivity.

◼Properties

▶The elements that lies above (K, Na,Ca,Mg And Al) and they replaces a other metals that lies below them in reactivity series.

▶The element in between the series are less reactive than above ones and are Zn, Fe, Pb, H, and Cu and replaces metals that lies below them

▶The element that lies are bottom are least reactive and gets replaced by all metals present above it that arr Hg and Ag.

$\underline \bold{Single \: displacement \: reaction}$

◼The reaction in which the less reactive metal in a compound when reacts with a reactive metal gets replaced by highly reactive metal.

So, for the Given reaction ,

◼Since,the Mg is more reactive than copper so copper gets replaced by magnesium and magnesium sulphate is formed.

$\large \boxed{ \bold{Mg + CuSO_4 \longrightarrow MgSO_4 + Cu}}$

Answer 2

$\large{\sf{\underline{\underline{Answer:}}}}$

$\sf CuSO_4(aq) + Mg(s) \to MgSO_4(aq) + Cu(s)$


$\large{\sf{\underline{\underline{Explanation:}}}}$

The ionic equation of this reaction shows the ions in this reaction dissociated in solution:

$\sf Cu^{2+} (aq) + SO^{2-}_4 (aq) + Mg(s) \\ \sf \: \: \: \: \: \to Mg^{2+} (aq) SO^{2-}_4 (aq) + Cu(s)$

The sulfate ion is a spectator ion - it does not react and remains in the aqueous phase during the reaction.

Copper is reduced into copper atoms which will precipitate out of solution. Magnesium is oxidised, and goes into the aqueous phase, effectively 'displacing' copper.