Write the folllowing redox rections using half equations
(i) `Zn(s) + PbCI_(2)(aq) rarr Pb(s)+ZnCI_(2)(aq)`
(ii)`2Fe^(3+)(aq)+2I^(-)(aq)rarrI_(2)(s)+2 Fe^(2+)(aq)`
(iii)`2Na(s)+CI_(2)(g)rarr2 NacI(s)`
(iv)`Mg(s)+CI_(2)(g)rarrMgCI_(2)(s)`
`(v)Zn(s)+2H^(+)(aq) rarr Zn^(2+)(aq)+H_(2)(g)`
In each of the reactions gien above mention
(a) Which reactant is oxidized ? to what ? (b) which reactant is hte oxidiser ? (c )which reactant is reduced ? To what ? (d) which reactant is hte reducer?

Explanation

(i) `Zn(s) rarr Zn^(2+)+2e^(-) ("oxidation") , Pb^(2+)(aq)+2e^(-) rarrPb(s)("reduction")`
Zn is oxidised to `Zn^(2+), Pb^(2+) ("reduction") , Pb^(2+)` is the oxidiser and Zn is the reducer
(ii) `2Fe^(3+)+2e^(-) rarr 2Fe^(2+) ("reduction") , 2I^(-)rarrI_(2)+2e^(-)("oxidation")`
`Fe^(3+)` reduced to `Fe^(2+) I^(-)` is oxidiased to `I_(2) , I^(-)` is the reducer and `Fe^(3+)` is the oxidiser
(iii)`2Na rarr2Na^(+)+2e^(-)("oxidation") , CI_(2)+2e^(-)rarr2CI^(-)`(reduction)
Na is oxidised to `Na^(+) "and" CI_(2)` is reduced to `CI^(-) , CI_(2)+2e^(-) rarr 2CI^(-)` (reduction )
Mg is oxidised o `Zn^(2+)` while `H^(+)` is reduced to `H_(2)` , Zn is ht reducer and `H^(+)` is the oxidiser