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The value closest to the thermal velocity of a Helium atom at room temperature $(300\,K)$in $ms^{-1}$ is $[k_B\, = 1 .4\times10^{-23}\,J/K;\, m_{He}\, = 7\times10^{-27}\,kg]$
A vessel is partitioned in two equal halves by a fixed diathermic separator. Two different ideal gases are filled in left $(L)$ and right $(R)$ halves. The rms speed of the molecules in $L$ part is equal to the mean speed of molecules in the $R$ part. Then the ratio of the mass of a molecule in $L$ part to that of a molecule in $R$ part is
$STATEMENT- 1$ The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5$ times the product of its pressure and its volume. because
$STATEMENT-2$ The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.
The temperature of an ideal gas at atmospheric pressure is $300\,K$ and volume $1\,m^3$. If temperature and volume become double, then pressure will be
The pressure $P,$ volume $V$ and temperature $T$ of a gas in the jar $A$ and the other gas in the jar $B$ at pressure $2P,$ volume $V/4$ and temperature $2T,$ then the ratio of the number of molecules in the jar $A$ and $B$ will be
The root mean square speed of molecules of nitrogen gas at $27^{\circ} C$ is approximately$.......m/s$(Given mass of a nitrogen molecule $=4.6 \times 10^{-26}\,kg$ and take Boltzmann constant $k _{ B }=1.4 \times 10^{-23}\,JK ^{-1}$ )
If hydrogen gas is heated to a very high temperature, then the fraction of energy possessed by gas molecules correspond to rotational motion ...........