NEET Chemistry States Of Matter MCQs

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:

A mixture of two diatomic ideal gases A and B, having molecular masses $m_A$ and $m_B$ respectively, is in thermal equilibrium. If $v_{rms,A}$ and $v_{rms,B}$ represent their root mean square speeds, what is the ratio of their most probable speeds ($v_{mp,A}/v_{mp,B}$)?

For a real gas at moderate pressure and temperature, the root mean square speed is found to be $v_{rms}$. How would $v_{rms}$ change if the gas were ideal and at the same temperature?

Ratio of root mean square speed of ${O_2}$ at 200 K and ${N_2}$ at 400 K will be

In deriving the kinetic equation we make use of the root mean square speed of the molecules which is:

The rms speed of hydrogen is $\sqrt 7$ times the rms speed of nitrogen. If $T$ is the temperature of the gas, then

If the rms speed of a gaseous molecule is $x\,\,{\rm{m}}{{\rm{s}}^{ - 1}}$ at a pressure $p$ atm, then what will be the rms speed at a pressure $2p$ atm and constant temperature

The root mean square speed of the molecules of diatomic gas is $u$. When the temperature is doubled, the molecules dissociates into two atoms. The new speed of the atom is:

The root mean square speed of the molecules of diatomic gas is $u$. When the temperature is doubled, the molecules dissociates into two atoms. The new speed of the atom is:

Which of the following gases would have the highest rms speed at 0\,^\circ C