For a given mass of a gas at constant temperature, the volume and the pressure are $V$ and $P$ respectively. Then the slope of the graph drawn between $\log_e V$ on the $X$-axis and $\log_e P$ on the $Y$-axis is

The mass of oxygen gas occupying a volume of $11.2 \text{ litres}$ at a temperature $27^{\circ}C$ and a pressure of $760 \text{ mm}$ of mercury in kilograms is $[$ Molecular weight of oxygen $= 32]$

The volume occupied by the molecules contained in $4.5 \, kg$ of water at $STP$,if the intermolecular forces vanish away,is ........ $m^{3}$.

The lowest pressure (the best vacuum) that can be created in the laboratory at $27^{\circ}C$ is $10^{-11} \; mm$ of $Hg$. At this pressure,the number of ideal gas molecules per $cm^{3}$ will be:

Two bulbs of identical volumes connected by a small capillary are initially filled with an ideal gas at temperature $T$. Bulb $2$ is heated to maintain a temperature $2 T$,while bulb $1$ remains at temperature $T$. Assume throughout that the heat conduction by the capillary is negligible. Then,the ratio of final mass of the gas in bulb $2$ to the initial mass of the gas in the same bulb is close to

If a given mass of gas occupies a volume of $10\, cc$ at $1\, atm$ pressure and a temperature of $100^{\circ}C$ $(373.15\, K)$,what will be its volume at $4\, atm$ pressure,assuming the temperature remains constant?