At $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be

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:

At $25 \, ^\circ C$ temperature and $760 \, mm \, Hg$ pressure,the volume of a gas is $600 \, mL$. Calculate the pressure when the volume of this gas becomes $640 \, mL$ at $10 \, ^\circ C$ temperature. Use the ideal gas equation: $\frac{p_1 V_1}{T_1} = \frac{p_2 V_2}{T_2}$

$A$ closed container is maintained at a constant temperature. It is first evacuated and then an ideal gas is continuously introduced into it. What will be the pressure of the gas inside the container?

The root mean square velocity of an ideal gas in a closed container of fixed volume is increased from $5 \times 10^4 \ cm \ s^{-1}$ to $10 \times 10^4 \ cm \ s^{-1}$. Which of the following statements correctly explains how the change is accomplished?

What will be the molar volume of nitrogen $(N_2)$ and argon $(Ar)$ at $273.15 \ K$ and $1 \ atm$?