At $1 \text{ atm}$ pressure and $0 \, ^oC$,a certain mass of a gas occupies $0.4 \, L$. Keeping the pressure constant,if the temperature is increased to $273 \, ^oC$,what will be its final volume (in $, L$)?

The molecular weights of $O_2$ and $SO_2$ are $32$ and $64$ respectively. If $1 \, L$ of $O_2$ at $15 \, ^\circ C$ and $750 \, mm$ pressure contains '$N$' molecules,the number of molecules in $2 \, L$ of $SO_2$ under the same conditions of temperature and pressure will be

$A$ certain mass of a gas occupies a volume of $2 \,L$ at $STP$. To what temperature must the gas be heated to double its volume, keeping the pressure constant?

The temperature at which $4 \ mol$ of a gas occupies $5 \ dm^3$ volume at $3.32 \ bar$ pressure is:

If $P, V, M, T,$ and $R$ represent pressure,volume,molar mass,temperature,and gas constant respectively,then the density of an ideal gas is given by:

$A$ sample of gas has a volume of $95 \, cm^3$ at a pressure of $9.962 \times 10^4 \, N m^{-2}$ and constant temperature. What will be its volume at $10.13 \times 10^4 \, N m^{-2}$ pressure at the same temperature (in $, cm^3$)?