(A) The oxidation state of sulfur in $Na_2S_2O_3$ changes from $+2$ to $+2.5$ in $Na_2S_4O_6$.The change in oxidation state per sulfur atom is $2.5 -

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(A) The oxidation state of sulfur in $Na_2S_2O_3$ changes from $+2$ to $+2.5$ in $Na_2S_4O_6$.The change in oxidation state per sulfur atom is $2.5 - 2 = 0.5$.Since there are $2$ sulfur atoms in one molecule of $Na_2S_2O_3$,the total change in oxidation state (n-factor) is $2 \times 0.5 = 1$.The equivalent weight $E$ is calculated as $E = \frac{\text{Molecular Weight}}{\text{n-factor}} = \frac{M}{1} = M$.

Class 11 Chemistry Some Basic Concepts of Chemistry Atomic, Molecular and Equivalent masses

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In the reaction $2Na_2S_2O_3 + I_2 \to Na_2S_4O_6 + 2NaI$,the equivalent weight of $Na_2S_2O_3$ (molecular weight = $M$) is equal to:

A
$M$
B
$M/2$
C
$M/3$
D
$M/4$

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Some Basic Concepts of Chemistry

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Atomic, Molecular and Equivalent masses

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Isotope	$\%$ Natural abundance	Molar mass
$^1H$	$99.985$	$1$
$^2H$	$0.015$	$2$

In the reaction $2Na_2S_2O_3 + I_2 \to Na_2S_4O_6 + 2NaI$,the equivalent weight of $Na_2S_2O_3$ (molecular weight = $M$) is equal to:

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In nature,carbon exists as a mixture of $C^{12}$ and $C^{13}$. The average atomic mass of carbon is $12.011$. What is the percentage abundance of $C^{12}$ in nature?

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Calculate the average atomic mass of hydrogen using the following data:

Isotope $\%$ Natural abundance Molar mass

$^1H$ $99.985$ $1$

$^2H$ $0.015$ $2$