A redox reaction involves oxidation of reductant liberating electrons, which are then consumed by an oxidant. The sum of two half reactions give rise to net redox change. In half reaction charge and atoms are always conserved.
In the reaction: `As_(2) S_(3) + HNO_(3) rarrH_(2)AsO_(4) +H_(2)SO_4, +NO` the element oxidised is:

Options

A. `Fe^(+8//3) to Fe^(+3) + 1/3 e`
B. `Fe^(+8//3) to Fe^(+2) - 2/3 e `
C. `(Fe^(+8//3))_3 to 3Fe^(+2)+ 2e`
D. `2(Fe^(+8//3))_3 to 3 (Fe^(+3))_2 + 2e`

Answer

D

Explanation

Electrons and atoms are conserved in half reaction .