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 $B$?

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 $[R=0.0821 \ L \ atm \ mol^{-1} \ K^{-1}]$

At $17\,^{\circ}C$ temperature,the volume of a gas is $400\, mL$. At what temperature will: $(i)$ the volume become double,and $(ii)$ the volume become half?

$A$ sample of gas occupies $100 \ mL$ at $27 \ ^oC$ and $740 \ mm$ pressure. When its volume is changed to $80 \ mL$ at $740 \ mm$ pressure,the temperature of the gas will be ............. $^oC$

At $400 \ K$,an ideal gas is enclosed in a $0.5 \ m^3$ vessel at a pressure of $203 \ kPa$. What is the change in temperature required (in $K$),if it occupies a volume of $0.2 \ m^3$ under a pressure of $304 \ kPa$? (Nearest integer)

For an ideal gas,which of the following graphs will not be a straight line?