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Question: Brine is electrolysed by using inert electrodes the reaction at anode is \_\_\_\_\_\_\_....

Brine is electrolysed by using inert electrodes the reaction at anode is _______.

A

Cl−(aq)⟶12Cl2( g)+e−;Ecell o=1.36 V\mathrm { Cl } ^ { - } { } _ { ( \mathrm { aq } ) } \longrightarrow \frac { 1 } { 2 } \mathrm { Cl } _ { 2 ( \mathrm {~g} ) } + \mathrm { e } ^ { - } ; \mathrm { E } _ { \text {cell } } ^ { \mathrm { o } } = 1.36 \mathrm {~V}

B

2H2O(l)⟶O2( g)+4H++4e−;Ecell 0=1.23 V2 \mathrm { H } _ { 2 } \mathrm { O } _ { ( \mathrm { l } ) } \longrightarrow \mathrm { O } _ { 2 ( \mathrm {~g} ) } + 4 \mathrm { H } ^ { + } + 4 \mathrm { e } ^ { - } ; \mathrm { E } _ { \text {cell } } ^ { 0 } = 1.23 \mathrm {~V}

C

D

H(aq )++e−⟶12H2( g);Ecell o=0.00 V\mathrm { H } _ { ( \text {aq } ) } ^ { + } + \mathrm { e } ^ { - } \longrightarrow \frac { 1 } { 2 } \mathrm { H } _ { 2 ( \mathrm {~g} ) } ; \mathrm { E } _ { \text {cell } } ^ { \mathrm { o } } = 0.00 \mathrm {~V}

Answer

Cl−(aq)⟶12Cl2( g)+e−;Ecell o=1.36 V\mathrm { Cl } ^ { - } { } _ { ( \mathrm { aq } ) } \longrightarrow \frac { 1 } { 2 } \mathrm { Cl } _ { 2 ( \mathrm {~g} ) } + \mathrm { e } ^ { - } ; \mathrm { E } _ { \text {cell } } ^ { \mathrm { o } } = 1.36 \mathrm {~V}

Explanation

Solution

Although reduction potential of O2\mathrm { O } _ { 2 } (i.e. water needs greater voltage for oxidation to O2\mathrm { O } _ { 2 } as it is a kinetically slow process.)