Question

Complete the following table of displacement reaction. Identify oxidising and reducing agents involved.

Reactants	Products
1. $Zn\left( S \right) + \,\_\_\_\_\_\left( {aq} \right)$	$\_\_\_\_\_\left( {aq} \right) + Cu\left( S \right)$
2. $Cu\left( S \right) + 2A{g^ + }\left( {aq} \right)$	$\_\_\_\_ + \_\_\_\_$

Answer 1

Hint : When the ions of a metal higher in the electrochemical series are combined with the ions of a metal lower in the electrochemical series, displacement reactions occur. The more reactive metal's atoms force their electrons onto the less reactive metal's ions.

Complete Step By Step Answer:
Reduction and oxidation (redox) reactions are chemical reactions that involve the exchange of electrons. When a chemical species loses electrons, it is said to be oxidised, and when it receives electrons, it is said to be reduced.
Now, coming to the question:
1. $Zn\left( S \right) + \,\_\_\_\_\_\left( {aq} \right) \to \_\_\_\_\left( {aq} \right) + Cu\left( S \right)$
In this reaction because zinc has a higher reactivity than copper, it replaces copper in a copper sulphate \[\left( {CuS{O_4}} \right)\] solution and creates zinc sulphate. The colour of the solution changes from blue to colourless during the operation.
The chemical equation of the reaction;
\[Zn{\text{ }} + {\text{ }}CuS{O_4}\; \to {\text{ }}ZnS{O_4}\; + {\text{ }}Cu\]
So, in this displacement reaction Copper sulphate $(CuS{O_4})$ acts as an oxidising agent by supplying oxygen to zinc, whereas zinc acts as a reducing agent by absorbing oxygen.
2. $Cu\left( S \right) + 2A{g^ + }\left( {aq} \right) \to \_\_\_\_ + \_\_\_\_$
In solution, copper metal became copper ions, while silver ions created silver metal.
\[Cu\left( s \right){\text{ }} + {\text{ 2}}A{g^ + }\left( {aq} \right)\; \to \;C{u^{2 + }}\left( {aq} \right){\text{ }} + {\text{ 2}}Ag\left( s \right)\;\]
\[Cu\left( s \right)\] ions lose electrons to become \[C{u^{2 + }}\left( {aq} \right)\] ions, while \[A{g^ + }\left( {aq} \right)\] ions gain electrons to become \[A{g^ + }\left( {aq} \right)\] ions . The \[Cu\left( s \right)\] loses electrons to be oxidized to \[C{u^{2 + }}\left( {aq} \right)\] . The \[A{g^ + }\left( {aq} \right)\] gain electrons to be reduced to \[Ag\left( s \right).\]

Note :
If the standard electrode potential for the redox reaction \[,{\text{ }}{E_{0\,\left( {\operatorname{Re} dox\,\,reaction} \right)}}\] , is positive, the redox reaction is spontaneous. The reaction will move forward if \[,{\text{ }}{E_{0\,\left( {\operatorname{Re} dox\,\,reaction} \right)}}\] is positive (spontaneous). We wouldn't anticipate the reverse reaction to be spontaneous after observing the spontaneous reaction of \[A{g^ + }\]and \[Cu\] . As a result, there is no interaction between \[Ag\] metal and\[C{u_2}^ + \].