The mass of oxygen gas occupying a volume of $11.2 \text{ litres}$ at a temperature $27^{\circ}C$ and a pressure of $760 \text{ mm}$ of mercury in kilograms is $[$ Molecular weight of oxygen $= 32]$

$A$ vessel contains $16 \,g$ of hydrogen and $128 \,g$ of oxygen at standard temperature and pressure $(STP)$. The volume of the vessel in $cm^{3}$ is:

If the pressure of a gas contained in a closed vessel is increased by $0.4\%$ when heated by $1\,^{\circ}C$,the initial temperature must be

$A$ jar $P$ is filled with a gas having pressure,volume,and temperature $P, V, T$ respectively. Another gas jar $Q$ is filled with a gas having pressure $2P$,volume $\frac{V}{4}$,and temperature $2T$. The ratio of the number of molecules in jar $P$ to those in jar $Q$ is:

An ideal gas is heated from $27^{\circ}C$ to $627^{\circ}C$ at constant pressure. If initial volume of gas is $4 \text{ m}^3$, then the new volume of the gas will be (in $\text{ m}^3$)

What is molar volume? Write its $SI$ unit.