Two separate bulbs contain ideal gases $A$ and $B$. The density of gas $A$ is twice that of gas $B$. The molecular mass of $A$ is half that of gas $B$. The two gases are at the same temperature. The ratio of the pressure of $A$ to that of gas $B$ is

What is the volume of $n$ moles of gas? Derive the formula for the combined gas law.

$N_2$ is found in a $1 \ L$ flask under $100 \ kPa$ pressure and $O_2$ is found in another $3 \ L$ flask under $320 \ kPa$ pressure. If the two flasks are connected,the resultant pressure is $............... \ kPa$.

$A$ sealed flask with a capacity of $2 \, dm^{3}$ contains $11 \, g$ of propane gas. The flask is so weak that it will burst if the pressure becomes $2 \, MPa$. The minimum temperature at which the flask will burst is $....... \, ^{\circ}C$. [Nearest integer] (Given: $R = 8.3 \, J \, K^{-1} \, mol^{-1}$. Atomic masses of $C$ and $H$ are $12 \, u$ and $1 \, u$ respectively.) (Assume that propane behaves as an ideal gas.)

$A$ syringe has a volume of $10.0 \text{ cm}^3$ at a pressure of $1 \text{ atm}$. If the end is sealed and the plunger is pushed down at a constant temperature, what will be the final volume when the pressure becomes $3.5 \text{ atm}$ (in $\text{ cm}^3$)?

$A$ certain sample of gas occupies a volume of $0.2 \ L$ at $0 \ ^oC$ and $1 \ \text{atm}$ pressure. What will be its volume at the same pressure but at $273 \ ^oC$ (in $L$)?