In the equation $PV = nRT$,the number of moles per liter can be expressed as:

The following graph illustrates:

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:

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

At $0\, ^\circ C$ and $1\, atm$ pressure,a gas occupies $100\, cc$. If the pressure is increased to $1.5$-times and temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be .............. $cc$.

$A$ sample of gas has a volume of $95 \, cm^3$ at a pressure of $9.962 \times 10^4 \, N m^{-2}$ and constant temperature. What will be its volume at $10.13 \times 10^4 \, N m^{-2}$ pressure at the same temperature (in $, cm^3$)?