Mass of one molecule of oxygen in $amu$ and in $gram$ respectively is

On reduction with hydrogen,$3.6 \, g$ of an oxide of a metal left $3.2 \, g$ of metal. If the equivalent weight of the metal is $32$,the simplest formula of the oxide would be:

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

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

Elements $X$ and $Y$ form compounds $X_2Y_3$ and $X_3Y_4$ respectively. If $0.2 \ mol$ of $X_2Y_3$ weighs $32.0 \ g$ and $0.4 \ mol$ of $X_3Y_4$ weighs $92.8 \ g$,then the atomic masses of $X$ and $Y$ are respectively:

The amount of $K_2Cr_2O_7$ (equivalent weight $49.04$) required to prepare $100 \ mL$ of its $0.05 \ N$ solution is ........ $g$.

Assertion : Equivalent weight of a base $= \frac{\text{Molecular weight}}{\text{Acidity}}$
Reason : Acidity is the number of replaceable hydrogen atoms in one molecule of the base.