$A$ gas occupies a volume of $300 \, cc$ at $27 \, ^\circ C$ and $620 \, mm$ pressure. The volume of gas at $47 \, ^\circ C$ and $640 \, mm$ pressure is......$cc$

The volume of a given mass of a gas is directly proportional to its Kelvin temperature at constant pressure. The above statement is known as . . . . . .

The density of a gas at $27\,^oC$ and $1\, atm$ is $d$. At constant pressure,at which of the following temperatures will its density become $0.75\, d$?

Explain the relationship between the moles of a gas,its volume,and its density.

If $2.5$ moles of an ideal gas at a certain temperature are allowed to expand isothermally and reversibly from an initial volume of $2$ $dm^3$ to $20$ $dm^3$, the work done by the gas is $-16.5$ $kJ$. The temperature (in $K$) of the gas is (Round off to the nearest value). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

The temperature of a flask is increased from $27\,^{\circ}C$ to $277\,^{\circ}C$. If $0.1\,dm^{3}$ of gas bubbles out from the flask at $277\,^{\circ}C$,calculate the volume of the flask. (in $,dm^{3}$)