Find the pressure of $5 \ mol$ $Cl_2$ gas filled in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

Find the pressure of a $CO_2$ gas when $6.022 \times 10^{22}$ molecules are placed in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

$A$ gas at $10^{\circ}C$ occupies a volume of $283 \text{ mL}$. If it is heated to $20^{\circ}C$ at constant pressure, what is the new volume of the gas (in $\text{ mL}$)?

Explain the mathematical formula,graph,and absolute zero temperature for Charles' Law.

The minimum pressure required to compress $600 \; dm^{3}$ of a gas at $1 \; bar$ to $150 \; dm^{3}$ at $40^{\circ} C$ is ......... $bar$.