The temperature of $4.0 \ mol$ of a gas occupying $5 \ dm^3$ at $3.32 \ bar$ is $(R = 0.083 \ bar \ dm^3 \ K^{-1} \ mol^{-1})$. (in $K$)

$A$ gas occupies a volume of $300 \ mL$ at $27 \ ^oC$ temperature and $730 \ mm$ pressure. What will be its volume at $STP$ in $mL$ (in $.2$)?

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:

Match the following gas laws with their respective equations.

At $STP$,$2 \ mol$ of $N_2$ gas in a $50 \ L$ container exhibits:

According to Charles's Law,what is the slope of the graph of volume versus temperature? ($V_0$ is the volume of the gas at $0\,^{\circ}C$ and $V_t$ is the volume of the gas at $t\,^{\circ}C$)