a An atomic gas molecule has only three transferable degrees of freedom.
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The volume of a gas at pressure $21 \times {10^4}\,N/{m^2}$ and temperature $27^o C$ is $83 $ litres. If $R = 8.3\ J/mol/K$, then the quantity of gas in $gm-mole$ will be
An ideal monoatomic gas is confined in a cylinder by a spring loaded piston of cross section $8.0\times10^{-3}\, m^2$ . Initially the gas is at $300\, K$ and occupies a volume of $2.4\times10^{-3}\, m^3$ and the spring is in its relaxed state as shown in figure. The gas is heated by a small heater until the piston moves out slowly by $0.1\, m$. The force constant of the spring is $8000\, N/m$ and the atmospheric pressure is $1.0\times10^5\, N/m^2$ . The cylinder and the piston are thermally insulated. The piston and the spring are massless and there is no friction between the piston and the cylinder. The final temperature of the gas will be: (Neglect the heat loss through the lead wires of the heater . The heat capacity of the heater coil is also negligible)
A thermally insulated vessel contains an ideal gas of molecular mass $M$ and ratio of specific heats $1.4$. Vessel is moving with speed $v$ and is suddenly brought to rest. Assuming no heat is lost to the surrounding and vessel temperature of the gas increases by ... ( $R =$ universal gas constant )
A gas consisting of a rigid diatomic molecules was initially under standard condition. Then, gas was compressed adiabatically to one$-$fifth of its initial volume. What will be the mean kinetic energy of a rotating molecule in the final state ?
Air is filled at $60^o C$ in a vessel of open mouth. The vessel is heated to a temperature $T$ so that $1/4^{th}$ part of air escapes. Assuming the volume of the vessel remaining constant, the value of $T$ is ....... $^oC$
One mole of a gas mixture is heated under constant pressure, and heat supplied $Q$ is plotted against temperature difference acquired. Find the approximate value of $\gamma $ for mixture
A gas at absolute temperature $300\,K$ has pressure $= 4 \times 10^{-10}\,N /m^2$ . Boltzmann constant, $k = 1.38 \times 10^{-23}\,J / K$ . The number of molecules per $cm^3$ is of the order of
If the root mean square velocity of the molecules of hydrogen at $NTP$ is $1.84\, km/s$. Calculate the root mean square velocity of oxygen molecule at $NTP$, molecular weight of hydrogen and oxygen are $2$ and $32$ respectively ....... $km/sec$