Hydrazine reacts with KIO_3 in the presence o | vedclass

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(D) The oxidation and reduction half-reactions are:Oxidation: $N_2H_4 \rightarrow N_2 + 4H^+ + 4e^-$Reduction: $IO_3^- + 6H^+ + Cl^- + 4e^- \rightarro

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$8, 53.5$

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(D) The oxidation and reduction half-reactions are:Oxidation: $N_2H_4 \rightarrow N_2 + 4H^+ + 4e^-$Reduction: $IO_3^- + 6H^+ + Cl^- + 4e^- \rightarrow ICl + 3H_2O$The equivalent mass is the molecular mass divided by the number of electrons gained or lost per molecule.For $N_2H_4$: Molecular mass = $32 \ g/mol$. Number of electrons lost = $4$.Equivalent mass of $N_2H_4 = \frac{32}{4} = 8$.For $KIO_3$: Molecular mass = $214 \ g/mol$. Number of electrons gained = $4$.Equivalent mass of $KIO_3 = \frac{214}{4} = 53.5$.

Isotope	Isotopic molar mass $(g \, mol^{-1})$	Abundance (%)
$^{36}Ar$	$35.96755$	$0.337$
$^{38}Ar$	$37.96272$	$0.063$
$^{40}Ar$	$39.9624$	$99.600$

Hydrazine reacts with $KIO_3$ in the presence of $HCl$ as:
$N_2H_4 + IO_3^- + 2H^+ + Cl^- \rightarrow ICl + N_2 + 3H_2O$
The equivalent masses of $N_2H_4$ and $KIO_3$ respectively are:

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Isotope Isotopic molar mass $(g \, mol^{-1})$ Abundance (%)

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Hydrazine reacts with $KIO_3$ in the presence of $HCl$ as:$N_2H_4 + IO_3^- + 2H^+ + Cl^- \rightarrow ICl + N_2 + 3H_2O$The equivalent masses of $N_2H_4$ and $KIO_3$ respectively are: