Question

What will be the equivalent load of $A{s_2}{S_3}$ in above reaction: (with sub-atomic mass of $A{s_2}{S_3}$ = $M$):
$28N{O_3}^ - $ + $3A{s_2}{S_3}$ + $4{H_2}O$ $ to $ $6As{O_4}^{3 - }$ + $28NO$ + $9S{O_4}^{2 - }$ + $8{H^ + }$
A.$\dfrac{M}{2}$
B.$\dfrac{M}{4}$
C.$\dfrac{M}{{24}}$
D.$\dfrac{M}{{28}}$

Answer 1

Hint:Oxidation province of $As$ changes from + 3 to +5. Subsequently, 1mol of $A{s_2}{S_3}$ loses two moles of electrons in this response. We can use the concept of finding equivalent mass of a particular compound just by having mass and change in oxidation state/number of that compound.

Complete step by step answer:
The oxidation number of arsenic in $A{s_2}{S_3}$ and in AsO43− is +3 and +5.
The adjustment in oxidation number per $As$molecule is 5 – 3 = 2.
The adjustment in oxidation number of 2 $As$ molecules is 2 × 2 = 4.
The equivalent mass of $A{s_2}{S_3}$ = formula mass of $A{s_2}{S_3}$ /absolute change in oxidation number of $As$
That is $\dfrac{M}{4}$.
So the correct answer of this particular question is option 2.

ADDITIONAL INFORMATION:
What is the concept of oxidation number/ oxidation state?
-Oxidation number of a molecule is characterized as the charge that a particle seems to have on framing ionic bonds with different heteroatoms. An ion having higher electronegativity (regardless of whether it shapes a covalent bond) is given a negative oxidation state.
The definition, doles out oxidation state to a molecule on conditions, that the particle –
Bonds with heteroatoms.
ii) Consistently structure ionic holding by either picking up or losing electrons, regardless of the real idea of holding.

Note:
Oxidation states, bigger than three, regardless of whether positive or negative are essentially incomprehensible. The superscript along sign is called the 'oxidation condition' of the molecule. Oxidation number is additionally alluded to as oxidation state. Various atoms have distinctive oxidation.