A container holds 4 g of helium at a pressure of 2 atm and a temperature of 300 K. If 8 g of oxygen is added to the container while maintaining the same volume and temperature, what is the new total pressure?

$5\,{\rm{g}}$ each of the following gases at 87\,^\circ C and $750\,{\rm{mm}}$ pressure are taken. Which of them will have the least volume?

At constant pressure, the temperature of an ideal gas is doubled. What happens to its volume?

When gases are heated from 20\,^\circ C to 40\,^\circ C at constant pressure, the volume:

A preweighted vessel was filled with ${\rm{C}}{{\rm{O}}_2}$ at STP and weighed. It was then evaluated, filled with ${\rm{S}}{{\rm{O}}_2}$ at the same temperature and pressure and again weighted. The weight of the ${\rm{C}}{{\rm{O}}_2}$ will be

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?

A closed vessel contains equal number of nitrogen and oxygen molecules at a pressure of $P$ mm. If nitrogen is removed from the system, then the pressure will be:

Slope between $pV\,\,{\rm{and}}\,\,p$ at constant temperature is

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

Ideal gas equation in terms of KE per unit Volume, E is

$10{\rm{g}}$ 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 $(at.{\rm{ }}Wt.{\rm{ }}of{\rm{ }}fluorine = 19)$