[" In the reaction; "],[As_(2)S_(3)+HNO_(3)rarr H_(3)AsO_(4)+H_(2)SO_(4)+NO],[" the element oxidized is/are :- "]

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:

Balance the equation : As_(2)S_(3) + HNO_(3) rarr H_(2)AsO_(3) + H_(2)SO_(4) + NO

As_(2)S_(3)+HNO_(3)toH_(3)AsO_(4)+H_(2)SO_(4)+NO the element which is oxidised in the reaction is / are

As_(2)S_(3)+HNO_(3)toH_(3)AsO_(4)+H_(2)SO_(4)+NO the element which is oxidised in the reaction is / are

In the reaction , As_2S_3+HNO_3 ➡ H_3AsO_4 +H_2SO_4 +NO, the element oxidised is/are:

Statement In the reactions , 3As_(2)S_(3)rarr28HNO_(3)+4H_(2)Orarr6H_(3)AsO_(4)+9H_(2)SO_(4)+28NO electrons transferred are 84 . Explanation As is oxidised from +3 to +5 and sulphur from -2 to +6

Assertion: In the reaction, 3As_(2)S_(3)+28HNO_(3)+4H_(2)O rarr 6H_(3)SAsO_(4)+9H_(2)SO_(4)+28NO electrons transferred are 84 . Reason: As is oxidised from +3 to +5 and sulphur from -2 to +6 .

In the reaction As_(2)S_(5)+xHNO_(3)rarr5H_(2)SO_(4)+yNO_(2)+2H_(3)AsO_(4) +12H_(2)O . The values of x and y are