In the reaction $SO_2 + 2H_2S \rightarrow 3S + 2H_2O$,the equivalent mass of the oxidizing agent is .....

$3.011 \times 10^{22}$ atoms of an element weigh $1.15 \ g$. The atomic mass of the element is: (in $amu$)

The equivalent weights of $H_3PO_4$ in the following reactions are respectively:
$H_3PO_4 + OH^{-} \rightarrow H_2PO_4^- + H_2O$
$H_3PO_4 + 2OH^{-} \rightarrow HPO_4^{2-} + 2H_2O$
$H_3PO_4 + 3OH^{-} \rightarrow PO_4^{3-} + 3H_2O$

$0.126 \ g$ of an acid requires $20 \ mL$ of $0.1 \ N$ $NaOH$ for complete neutralization. The equivalent weight of the acid is:

Calculate the molar mass of the following:
$(i)$ $H_2O$
$(ii)$ $CO_2$
$(iii)$ $CH_4$

$0.16 \ g$ of dibasic acid required $25 \ mL$ of decinormal $NaOH$ solution for complete neutralization. The molecular weight of the acid will be: