Question

For the following redox reaction write a balanced equation for the whole reaction and include states of matter MnO4^- (aq) + Cl ^- (aq) -> Mn^2+ (aq) + Cl2 (g)

Answer 1

Lets balance this reaction step by step

1).Balanced oxidation and reduction.

2 Cl ^- (aq) --- > Cl2 (g)

MnO4^- (aq) -> Mn^2+ (aq)

2) Balancing O and H : This is done by using H2O molecule

2 Cl ^- (aq) --- > Cl2 (g)

MnO4^- (aq)+ 8 H+ (aq)   -> Mn^2+ (aq) + 4 H2O (l)

3) Charge balance : This is done by using electrons.

2 Cl ^- (aq) --- > Cl2 (g) + 2e-

MnO4^- (aq)+ 8 H+ (aq)+ 5e-   -> Mn^2+ (aq) + 4 H2O (l)

4) electron balancing

10 Cl ^- (aq) --- >5 Cl2 (g) + 10e-

2 MnO4^- (aq)+ 16 H+ (aq)+ 10e-   -> 2 Mn^2+ (aq) + 8 H2O (l)

5) Addition of oxidation and reduction half

10 Cl ^- (aq) --- >5 Cl2 (g) + 10e-

2 MnO4^- (aq)+ 16 H+ (aq)+ 10e-   -> 2 Mn^2+ (aq) + 8 H2O (l)

----------------------------------------------------------------

2 MnO4- + 10Cl- + 16 H+ (aq) --- > 5 Cl2 (g) + 2 Mn²⁺ (aq) + 8 H2O (l)

Balanced equation

2 MnO4- + 10Cl- + 16 H+ (aq) --- > 5 Cl2 (g) + 2 Mn²⁺ (aq) + 8 H2O (l)