If the density of gas $A$ is $1.5$ times that of gas $B$,and the molecular mass of $A$ is $M$,then the molecular mass of $B$ is:

At $0\, ^\circ C$ and $1\, \text{atm}$ pressure,a gas occupies $100\, \text{cc}$. If the pressure is increased to $1.5$ times and the temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be :- $cc$

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of $1 \, atm$ but also a concentration of $1 \, mol \, L^{-1}$ $(R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1})$?

$100 \, g$ of an ideal gas is kept in a cylinder of $416 \, L$ volume at $27^{\circ} C$ under $1.5 \, bar$ pressure. The molar mass of the gas is $.... \, g \, mol^{-1}$. (Nearest integer) (Given : $R = 0.083 \, L \, bar \, K^{-1} \, mol^{-1}$)

Two separate bulbs contain ideal gases $A$ and $B$. The density of gas $A$ is $4$ times 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

At $17\,^{\circ}C$ temperature,the volume of a gas is $400\, mL$. At what temperature will: $(i)$ the volume become double,and $(ii)$ the volume become half?