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A flask contains Hydrogen and Argon in the ratio $2: 1$ by mass. The temperature of the mixture is $30^{\circ} C$. The ratio of average kinetic energy per molecule of the two gases ( $K$ argon/ $K$ hydrogen) is: (Given: Atomic Weight of $Ar = 39.9$)
If $\mathrm{n}$ is the number density and $\mathrm{d}$ is the diameter of the molecule, then the average distance covered by a molecule between two successive collisions (i.e. mean free path) is represented by :
The rms speed of oxygen molecule in a vessel at particular temperature is $\left(1+\frac{5}{x}\right)^{\frac{1}{2}} v$, where $v$ is the average speed of the molecule. The value of $x$ will be:(Take $\pi=\frac{22}{7}$ )
The value of the gas constant $(R)$ calculated from the perfect gas equation is $8.32\, joules/gm \,mole\, K,$ whereas its value calculated from the knowledge of ${C_P}$ and ${C_V}$ of the gas is $1.98\, cal/gm\, mole\, K.$ From this data, the value of $J$ is ......... $J/cal$
A vessel contains $1$ mole of $O_2$ gas (molar mass $32$) at a temperature $T$. The pressure of the gas is $P$. An identical vessel containing one mole of $He$ gas (molar mass $4$) at a temperature $2T$ has a pressure of
The relation between root mean square speed $\left( v _{ rms }\right)$ and most probable speed $\left( v _{ p }\right)$ for the molar mass $M$ of oxygen gas molecule at the temperature of $300\, K$ will be