$A$ certain mass of a gas occupies a volume of $2 \ dm^{3}$ at $STP$. At what temperature will the volume of the gas become double,keeping the pressure constant (in $^{\circ} C$)?

Which one of the following indicates the correct value of the gas constant $R$?

Equal volumes of two gases which do not react together are enclosed in separate vessels. Their pressures are $100 \ mm$ and $400 \ mm$ respectively. If the two vessels are joined together,then what will be the pressure of the resulting mixture (temperature remaining constant)?

$A$ gas obeys Charles's law in the temperature range $0-500 \ K$ at a given pressure. Its volume changes to zero at a temperature of:

$A$ home owner uses $4.00 \times 10^{3} \ m^{3}$ of methane $(CH_{4})$ gas (assume $CH_{4}$ is an ideal gas) in a year to heat his home. Under the pressure of $1.0 \ atm$ and $300 \ K$,the mass of gas used is $X \times 10^{5} \ g$. The value of $X$ is $.......$ (Nearest integer).
(Given $R = 0.083 \ L \ atm \ K^{-1} \ mol^{-1}$)

Which of the following does not represent Charles's Law?