Write the following redox reactions using half equations:
a. `Zn(s)+PbCl_(2)(aq)rarrPb(s)+ZnCl_(2)(aq)`.
b. `2Fe^(3+)(aq)+2I^(ө)(aq)rarrI_(2)(aq)+2Fe^(2+)(aq)`
c. `2Na(s)+Cl_(2)(g)rarr2NaCl(s)`
d. `Mg(s)+Cl_(2)(g)rarrMgCl_(2)(s)`
e. `Zn(s)+2H^(o+)(aq)rarrZn^(2+)(aq)+H_(2)(g)` .

Answer

A

Explanation

a. `Zn(s)rarrZn^(2+)(aq)+2e^(-)`(oxidation)
`Pb^(2+)(aq)+2e^(-)rarrPb(s)`(reduction)
b. `2Fe^(3+)(aq)+2e^(-)rarr2Fe^(2+)(aq)` (reduction)
`2I^(-)(aq)rarrI_(2)(aq)+2e^(-)`(reduction)
c. `2Na(aq)rarr2Na^(o+)(aq)+2e^(-)`(oxidation)
`Cl_(2)(g)+2e^(-)rarr2Cl^(ө)(aq)`(reduction)
d. `Mg(s)rarrMg^(2+)(aq)+2e^(-)`(oxidation)
`Cl_(2)(g)+2e^(-)rarr2Cl^(ө)` (reduction)
e. `Zn(s)rarrZn^(2+)(aq)+2e^(-)` (oxidation)
`2H^(o+)(aq)+2e^(-)rarrH_(2)(g)` (reduction)