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

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 : SO_(2) + Na_(2)CrO_(4) + H_(2)SO_(4) rarr Na_(2)SO_(4) + Cr_(2)(SO_(4))_(3) + H_(2)O

Balance the following equations. 2) H_(2)O_(2)rarr H_(2)O+O_(2)

How many electrons are transferred from reductant to oxidant is the following redox As_(2)S_(3) + HNO_3 rarr H_3ASO_(4) + H_2SO_4+NO

Balance the follwowing equations. 1) Al(OH)_(3)rarr Al_(2)O_(3)+H_(2)O

What is the mole coefficient of H_(2)SO_(4) in the balanced equation. K_(2)Cr_(2)O_(7) + FeSO_(4) + H_(2)SO_(4) rarr K_(2)SO_(4) + Fe_(2)(SO_(4))_(3) + Cr_(2)(SO_(4))_(3) + H_(2)O

Balance the follwowing equations. 5) NaOH +H_(2)SO_(4) rarr Na_(2)SO_(4)+H_(2)O

The equivalent weights of oxidising and reducing agents can be calculated by the number of electrons gained or lost. The equivalent weight of an oxidising agent is the number of parts by weight of the substance which gains one electron. Thus, it is equal to the molecular weight of the substance divided by the number of electrons gained in the balanced chemical equation. Similarly, equivalent weight of a reducing agent is equal to the molecular weight divided by the number of electrons lost as represented in the balanced chemical equation The equivalent weght of As_(2),S_3 in the following reaction As_(2)S_(3) + H^(+) + NO_(3)^(-) rarr NO + H_(2)O + AsO_(4)^(3-) + SO_(4)^(2-) is related to its molecular weight as

Balance the following chemical equation. C_(2)H_(6)+O_(2)rarr CO_(2)+H_(2)O