Some amount of dichloromethane $\left({\mathrm{CH}}_2{\mathrm{Cl}}_2\right)$ is added to $671.141\mathrm{mL}$ of chloroform $\left({\mathrm{CHCl}}_3\right)$ to prepare $2.6\times {10}^{-3}\mathrm{M}$ solution of ${\mathrm{CH}}_2{\mathrm{Cl}}_2\left(\mathrm{DCM}\right)$. The concentration of $\mathrm{DCM}$ is _____ ppm (by mass).

Given: Atomic mass : $\mathrm{C}=12;\mathrm{H}:1;\mathrm{Cl}=35.5$ density of ${\mathrm{CHCl}}_3=1.49\mathrm{g} {\mathrm{cm}}^{-3}$

Assume carbon burns according to following equation :
$2\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2( \mathrm{g})\to 2\mathrm{CO}\text{ (s) }$
when $12 \mathrm{g}$ carbon is burnt in $48 \mathrm{g}$ of oxygen, the volume of carbon monoxide produced is $\_\_\_\_\_\_\times {10}^{-1} \mathrm{L}$ at STP [nearest integer]

[Given : Assume $\mathrm{CO}$ as ideal gas, Mass of $\mathrm{C}$ is $12 \mathrm{g} {\mathrm{mol}}^{-1}$, mass of $O$ is $16 \mathrm{g} {\mathrm{mol}}^{-1}$ and molar volume of an idal gas at STP is $22.7 \mathrm{L} {\mathrm{mol}}^{-1}$ ]

The density of $3\mathrm{M}$ solution of $\mathrm{NaCl}$ is $1.0 \mathrm{g} {\mathrm{mL}}^{-1}$. Molality of the solution is $\_\_\_\_\_\_\times {10}^{-2} \mathrm{m}$ (Nearest integer).

Given: Molar mass of $\mathrm{Na}$ and $\mathrm{Cl}$ is $23$ and $35.5 \mathrm{g}$ ${\mathrm{mol}}^{-1}$ respectively.

The molality of a $10\%(\mathrm{v}/\mathrm{V})$ solution of di-bromine solution in ${\mathrm{CCl}}_4$ (carbon tetrachloride) is $\mathrm{x}$ '. $\mathrm{x}=$ $\_\_\_\_\_\times {10}^{-2}\mathrm{M}$. (Nearest integer)

[Given : molar mass of ${\mathrm{Br}}_2=160 \mathrm{g} {\mathrm{mol}}^{-1}$

atomic mass of $\mathrm{C}=12 \mathrm{g} {\mathrm{mol}}^{-1}$

atomic mass of $\mathrm{Cl}=35.5 \mathrm{g} {\mathrm{mol}}^{-1}$

density of dibromine $=3.2 \mathrm{g} {\mathrm{cm}}^{-3}$

density of $\left.{\mathrm{CCl}}_4=1.6 \mathrm{g} {\mathrm{cm}}^{-3}\right]$