$0.1 \ g$ of metal combines with $46.6 \ mL$ of oxygen at $STP$. The equivalent weight of the metal is:

$16.25 \ g$ of metal chloride is obtained on complete conversion of $8 \ g$ of metal oxide into metal chloride. What will be the equivalent weight of the metal?

If the mass of an electron is halved,the mass of a proton is doubled,and the mass of a neutron is $3/4$ of its original mass,then what will be the new atomic mass of an $O^{16}$ atom?

An element of mass $A_1 \, g$ gives a chloride of mass $A_2 \, g$. Calculate its equivalent mass.

$A$ metal $M$ (specific heat $0.16 \ J \ g^{-1} \ K^{-1}$) forms a metal chloride with $65\%$ chlorine present in it. The formula of the metal chloride will be:

$5 \, mol$ of $AB_2$ weigh $125 \times 10^{-3} \, kg$ and $10 \, mol$ of $A_2B_2$ weigh $300 \times 10^{-3} \, kg$. The molar mass of $A$ $(M_A)$ and molar mass of $B$ $(M_B)$ in $kg \, mol^{-1}$ are: