Calculation of equivalent weight of oxidising agent
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To calculate the n-factor, we first find the oxidation states of the elements in both reactant and product side and identify the ones which undergo a change in oxidation state.
The oxidation state of Fe changes from +2 to +3. FeSO4 acts as a reducing agent. There is no change in the oxidation state of any element in SO4(2-). Therefore, the n-factor of FeSO4 is 3–2= 1
The oxidation state of Cl changes from +5 to -1. KClO3 acts as an oxidising agent. There is no change in the oxidation state of K and O. Therefore, the n-factor of KClO3 is 5-(-1)= 6
Equivalent weight = Molecular weight/n-factor
We can find the molecular weight of the reactants easily and now we know the n-factor of each of the reactants. So just plug in the values and find out the equivalent weight of each of the reactants.
The oxidation state of Fe changes from +2 to +3. FeSO4 acts as a reducing agent. There is no change in the oxidation state of any element in SO4(2-). Therefore, the n-factor of FeSO4 is 3–2= 1
The oxidation state of Cl changes from +5 to -1. KClO3 acts as an oxidising agent. There is no change in the oxidation state of K and O. Therefore, the n-factor of KClO3 is 5-(-1)= 6
Equivalent weight = Molecular weight/n-factor
We can find the molecular weight of the reactants easily and now we know the n-factor of each of the reactants. So just plug in the values and find out the equivalent weight of each of the reactants.
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Find the n factor of oxidising agent by calculating oxidation number before and after reduction
then eq wt = wt/ change in oxidation number
then eq wt = wt/ change in oxidation number
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