A vessel contains an ideal gas at pressure P and temperature T. If the root mean square speed of the gas molecules doubles, keeping the volume constant, the new pressure P' will be:

Oxygen gas generated by the decomposition of potassium chlorate is collected. The volume of oxygen collected at 24\,^\circ C and atmospheric pressure of 760 mm Hg is 128 mL. Calculated the mass of oxygen gas obtained. The pressure of the water vapour at 24\,^\circ C is 22.4 mm Hg

380 mL of a gas at 27\,^\circ C , 800 mm of Hg weighs 0.455 g. The molecular weight of gas is

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:

Which law states that the pressure of a gas is inversely proportional to its volume at constant temperature?

What is the value of the ideal gas constant (R) in L atm/mol K?

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?

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

The pressure of gas having 2 mole in $44.8{\rm{litre}}$ vessel at $540{\rm{K}}$ is:

A mixture of 1 mol of He and 1 mol of CO$_2$ is contained in a vessel of volume V at 20°C. If the mixture behaves ideally, what is the pressure exerted by He?