For an ideal gas,the number of moles per litre in terms of its pressure $P$,gas constant $R$,and temperature $T$ is:

Containers $A$ and $B$ contain the same gas. If the pressure,volume,and temperature of container $A$ are all twice those of container $B$,what is the ratio of the number of molecules in $A$ to those in $B$?

In the gas equation $PV = nRT$,the universal gas constant $R$ depends on:

How many moles of $He$ gas occupy $22.4 \, L$ at $30^{\circ}C$ and $1 \, atm$ pressure?

If $2.5$ moles of an ideal gas at a certain temperature are allowed to expand isothermally and reversibly from an initial volume of $2$ $dm^3$ to $20$ $dm^3$, the work done by the gas is $-16.5$ $kJ$. The temperature (in $K$) of the gas is (Round off to the nearest value). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

The nitrogen gas pressure inside a container of volume $2.6 \ cm^3$ is $2.3 \ atm$ at $27^{\circ} C$. The approximate number of moles of nitrogen present in the container is $[R=0.0821 \ L \ atm \ mol^{-1} \ K^{-1}]$