What is the volume of a gas at $1.032 \times 10^5 \ Nm^{-2}$ if it occupies $1 \ dm^3$ of volume at normal temperature and pressure (in $dm^3$)?

An ideal gas expands isothermally and reversibly from $10 \ m^3$ to $20 \ m^3$ at $300 \ K$,performing $5.187 \ kJ$ of work on the surroundings. Calculate the number of moles of gas used.

$3.4$ moles of an ideal gas occupies a volume of $68 \ mL$ at $300 \ K$. What would be the pressure of the gas? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

$400 \ cm^{3}$ of oxygen at $27\,^{\circ}C$ were cooled to $-3\,^{\circ}C$ without change in pressure. The contraction in volume will be ............... $cm^{3}$

Derive the relation between density $(d)$ and molar mass $(M)$ for an ideal gas.

$A$ 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 $\text{ mL}$)?