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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 $({\gamma _{{O_2}}} = 1.4,\,\,{\gamma _{C{O_2}}} = 1.3)$
$5$ moles of oxygen is heated at constant volume from $10°C$ to $20°C.$ The change in the internal energy of the gas is (the gram molecular specific heat of oxygen at constant pressure...... $cal$ ${C_p} = 8$ $cal/mole \,°C$ and $R = 8.3 cal/mole\, °C)$
The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from ${0^o}C$ to ${100^o}C$ at constant pressure. The amount of heat delivered will be ...... $cal$
A sample of an ideal gas occupies a volume $V$ at a pressure $P$ and absolute temperature $T,$ the mass of each molecule is $m.$ The expression for the density of gas is ($k =$ Boltzmann’s constant)
The temperature of an ideal gas is increased from $200\,K$ to $800\,K$. If r.m.s. speed of gas at $200\,K$ is $v_0$. Then, r.m.s. speed of the gas at $800\,K$ will be:
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