1.0 L of ${N_2}$ and 7/8 L of ${O_2}$ at the same temperature and pressure were mixed together. What is the relation between the masses of the two gases in the mixture?

An ideal gas expands according to $PV =$ constant. On expansion, the temperature of gas:

Which gas has the highest partial pressure in atmosphere?

The density of ${N_2}$ gas at 0.821 atmospheric pressure and ${7^0}C$

A perfect gas of a given mass is heated first in a small vessel and then in a large vessel, such that their volume remains unchanged. The $P - T$ curves are:

If two moles of a ideal gas at 546 K occupy volume 44.8 L, then pressure must be

A perfect gas of a given mass is heated first in a small vessel and then in a large vessel, such that their volume remains unchanged. The $P - T$ curves are:

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

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

Under identical condition of temperature and pressure, which among the following gases has lowest density?

At NTP, the density of a gas, whose molecular weight is 45, is