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Considering the gases to be ideal, the value of $\gamma = \frac{{{C_P}}}{{{C_V}}}$ for a gaseous mixture consisting of $= 3$ moles of carbon dioxide and $2$ moles of oxygen will be $({\gamma _{{O_2}}} = 1.4,\,\,{\gamma _{C{O_2}}} = 1.3)$
One mole of an ideal monatomic gas requires $210 \,J$ heat to raise the temperature by $10\, K$, when heated at constant temperature. If the same gas is heated at constant volume to raise the temperature by $10\, K$ then heat required is ....... $J$
A mixture of one mole of monoatomic gas and one mole of a diatomic gas (rigid) are kept at room temperature $\left(27^{\circ} \mathrm{C}\right)$. The ratio of specific heat of gases at constant volume respectively is:
A closed vessel contains $8\,gm$ of oxygen and $7\,gm$ of nitrogen. The total pressure is $10\, atm$ at a given temperature. If now oxygen is absorbed by introducing a suitable absorbent the pressure of the remaining gas in atm will be
An ideal gas filled in a cylinder occupies volume $V$. The gas is compressed isothermally to the volume $V/3$. Now, the cylinder valve is opened and the gas is allowed to leak keeping temperature same. What percentage of the number of molecules should escape to bring the pressure in the cylinder back to its original value?