Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
The number of molecules in one litre of an ideal gas at $300 \,{K}$ and $2$ atmospheric pressure with mean kinetic energy $2 \times 10^{-9}\, {J}$ per molecules is $....\, \times 10^{11}$
If the intermolecular forces vanish away, the volume occupied by the molecules contained in $4.5 \,kg$ water at standard temperature and pressure will be
Vessel $A$ is filled with hydrogen while vessel $B,$ whose volume is twice that of $A,$ is filled with the same mass of oxygen at the same temperature. The ratio of the mean kinetic energies of hydrogen and oxygen is
In the two vessels of same volume, atomic hydrogen and helium at pressure $1\, atm$ and $2\, atm$ are filled. If temperature of both the samples is same, then average speed of hydrogen atoms $ < {C_H} > $ will be related to that of helium $ < {C_{He}} > $ as
The number density of molecules of a gas depends on their distance $r$ from the origin as, $n\left( r \right) = {n_0}{e^{ - \alpha {r^4}}}$. Then the total number of molecules is proportional to
Two vessels $A$ and $B$ are of the same size and are at same temperature. A contains $1 \mathrm{~g}$ of hydrogen and $B$ contains $1 \mathrm{~g}$ of oxygen. $\mathrm{P}_{\mathrm{A}}$ and $\mathrm{P}_{\mathrm{B}}$ are the pressures of the gases in $A$ and $\mathrm{B}$ respectively, then $\frac{\mathrm{P}_{\mathrm{A}}}{\mathrm{P}_{\mathrm{B}}}$ is: