An ideal gas undergoes a process in which its pressure P and volume V are related by $PV^n = constant$, where n is a constant. If the gas expands adiabatically ($n = \gamma$, where $\gamma = C_P/C_V$), which of the following statements is TRUE regarding the work done by the gas?

When air is blown to balloon (at constant temperature) its pressure and volume both increases. This violates:

One poise is equal to:

Calculate the pressure in bar exerted by 128 g of oxygen gas contained in a 20.0 L vessel at a temperature of $27^\circ C$, assuming ideal gas behavior. (Use $R = 0.0831\ L\ bar\ K^{-1}\ mol^{-1}$)

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of $1{\rm{mol}}\,\,{\rm{litr}}{{\rm{e}}^{ - 1}}$ ? $(\;R = 0.082$ litre atm ${\rm{mo}}{{\rm{l}}^{ - 1}}{\deg ^{ - 1}})$

$10{\rm{g}}$ of hydrogen fluoride gas occupy 5.6 litre of volume at NTP. The empirical formula of the gas is HF. The molecular formula of the gas will be $(at.{\rm{ }}Wt.{\rm{ }}of{\rm{ }}fluorine = 19)$

The density of a gas is 1.964 g $d{m^{ - 3}}$ at 273 K and 76 cm Hg. The gas is

A $0.5\,\,{\rm{d}}{{\rm{m}}^3}$ flask contains gas $A$ and another flask of ${\rm{1}}\,\,{\rm{d}}{{\rm{m}}^{\rm{3}}}$ contains gas $B$ at the same temperature. If density of gas $A$ is $3.0\,\,{\rm{g}}\,{\rm{d}}{{\rm{m}}^{ - 3}}$  and of gas $B\,\,is\,\,1.5\,\,{\rm{g}}\,{\rm{d}}{{\rm{m}}^{ - 3}}$  and ${\rm{mol}}.{\rm{wt}}.{\rm{of}}\,A = \frac{1}{2}{\rm{mol}}.\,\,{\rm{wt}}.\,\,{\rm{of}}\,\,B$,  then the ratio of pressure exerted by gases is:

Gas equation $PV = nRT$ is obeyed by:

A gas at 298 K is shifted from a vessel of $250\,\,{\rm{c}}{{\rm{m}}^3}$ capacity to that of 1 L capacity. The pressure of the gas will

An open vessel at 27\,^\circ C  is heated until 3/8th of the air in it has been expelled. Assuming that the volume remains constant, calculate the temperature at which the vessel was heated