Explain the feasibility of the following reaction: `Zn+Cu^(2+)rarrZn^(2+)+Cu` [Given: `Zn^(2+)|Zn` and `Cu^(2+)|Cu` redox couples have the standard electrode potential of `-0.76V and +0.34V,` respectively.]

Explanation

Half reactions for the given redox reaction are :
Oxidation (or anode) reaction:
`Zn(s)rarr Zn^(2+)(aq)+2e , E_("anode")^(@)=-0.76V`
Reduction (or cathode) reaction,
`Cu^(2+)(aq)+2e rarr Cu(s), E_("anode")^(@)=+0.34V`
Net reaction : `Zn(s)+Cu^(2+)(aq)rarr Cu(s)+Zn^(2+)(aq)" ....[1]"`
For this reaction, `E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)`
`=[0.34-(-0.76)]V=1.1V`
Since `E_("cell")^(@) gt0`, reaction (1) is feasible under standard conditions.