The temperature of $1 \, mol$ of a gas is increased by $2 \, ^oC$ at constant pressure. The work done will be:

The graph that does not represent the behaviour of an ideal gas is

If $P, V, M, T,$ and $R$ represent pressure,volume,molar mass,temperature,and gas constant respectively,then the density of an ideal gas is given by:

An evacuated glass vessel weighs $40.0 \ g$ when empty,$135.0 \ g$ when filled with a liquid of density $0.95 \ g \ mL^{-1}$ and $40.5 \ g$ when filled with an ideal gas at $0.82 \ atm$ at $250 \ K$. The molar mass of the gas in $g \ mol^{-1}$ is .... .
(Given : $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$ )

Three flasks of equal volumes contain $CH_4$,$CO_2$,and $Cl_2$ gases respectively. They will contain equal number of molecules if

$A$ gas occupies $100 \, cc$ volume at $0 \, ^oC$ temperature and $1 \, atm$ pressure. If the pressure is increased by $1.5$ times and the temperature is increased by one-third of its absolute temperature,what will be the final volume of the gas in $cc$?