$A$ 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:

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 $, L$)?

Pure hydrogen sulphide is stored in a tank of $100 \, L$ capacity at $20 \, ^oC$ and $2 \, atm$ pressure. The mass of the gas will be ............... $g$.

How many moles of dioxygen are present in $8.314 \times 10^{-3} \ m^3$ of it at $318 \ K$ having pressure $3.18 \times 10^5 \ N \ m^{-2}$ (in $mole$)? $(R=8.314 \ J \ K^{-1} \ mol^{-1})$

If the density of neon gas at $350 \ K$ is $0.9 \ g \ L^{-1}$,calculate the pressure of the gas. (in $bar$)

The density of a gas $A$ is three times that of a gas $B$. If the molecular mass of $A$ is $M$,the molecular mass of $B$ is: