Calculate the pressure of $1.5 \ mol$ of gas having volume $3 \ dm^3$ at $300 \ K$ $(R=0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1})$. (in $atm$)

Find the gas,if its density at $273 \ K$ temperature and $76 \ cm \ Hg$ pressure is $1.94 \ g / dm^3$.

Volume occupied by a gas at $1 \, \text{atm}$ pressure and $0 \, ^\circ C$ is $V \, mL$. Its volume at $273 \, K$ will be

The volume-temperature graph of a given mass of an ideal gas at constant pressure is shown below. What is the correct order of pressures?

When $48 \, L$ of dry $N_2$ gas is passed through $36 \, g$ of $H_2O$ at $27 \, ^oC$,the weight of water decreases by $1.20 \, g$. What is the vapor pressure of water in $atm$?

Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in the figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is kept constant. The partial pressures of $A$ and $B$ respectively (in $atm$) are: