If $74.5 \ g$ of a metallic chloride contains $35.5 \ g$ of chlorine,then the equivalent mass of the metal will be ...... .

Calculate the molar mass of naturally occurring argon from the data given in the following table:

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

$71 \ g$ of chlorine combines with a metal to form $111 \ g$ of its chloride. The chloride is isomorphous with $MgCl_2 \cdot 6H_2O$. The atomic weight of the metal is:

An oxide of an element contains $67.67\%$ oxygen and the vapour density of its volatile chloride is $79$. What is the atomic weight of the element?

The specific heat of a metal is $0.031 \ cal \ g^{-1} \ ^\circ C^{-1}$ and its equivalent weight is $103.6$. What is the exact atomic weight of the metal?

If the molar mass of phosphoric acid $\left[ H_3PO_4 \right]$ is $98 \ g/mol$,calculate the atomic mass of $P$. (in $g/mol$)