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:

What is the molar volume of an ideal gas at $STP$ (or $NTP$) and $SATP$?

At $300 \ K$ temperature and $1 \ atm$ pressure,the weight of $1 \ L$ of a gas is $2 \ g$. If the pressure is changed to $0.75 \ atm$,at what temperature in $K$ will the weight of $1 \ L$ of the same gas be $1 \ g$?

What will be the effect on the density of $0.09 \ mol$ of a gas at $300 \ K$ if its pressure is increased?

At the same temperature,gas $A$ is taken in a $0.5 \, dm^3$ flask and gas $B$ is taken in a $1 \, dm^3$ flask. If the density of $A$ is $3.0 \, g \, dm^{-3}$ and that of $B$ is $1.5 \, g \, dm^{-3}$,and the molar mass of $A$ is $1/2$ of $B$,what is the ratio of the pressures exerted by the gases?

Match the following graphs of an ideal gas with their respective axes ($X$ and $Y$).
$(A)$ $P$ vs $V$ (at constant $T$)
$(B)$ $V$ vs $T$ (at constant $P$)
$(C)$ $P$ vs $T$ (at constant $V$)
List-$I$:
$(1)$ $P$ on $Y$-axis,$T$ on $X$-axis
$(2)$ $P$ on $Y$-axis,$1/V$ on $X$-axis
$(3)$ $V$ on $Y$-axis,$T$ on $X$-axis