A gas mixture consists of 2 moles of O_2 and | vedclass

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(D) The internal energy $U$ of $n$ moles of an ideal gas is given by $U = \frac{f}{2} nRT$,where $f$ is the number of degrees of freedom.For $O_2$ (di

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$11$

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(D) The internal energy $U$ of $n$ moles of an ideal gas is given by $U = \frac{f}{2} nRT$,where $f$ is the number of degrees of freedom.For $O_2$ (diatomic gas),the number of degrees of freedom $f_1 = 5$ (neglecting vibrational modes).Internal energy of $2$ moles of $O_2$ is $U_1 = \frac{5}{2} 	imes 2 	imes RT = 5 RT$.For $Ar$ (monatomic gas),the number of degrees of freedom $f_2 = 3$.Internal energy of $4$ moles of $Ar$ is $U_2 = \frac{3}{2} 	imes 4 	imes RT = 6 RT$.The total internal energy of the system is $U_{total} = U_1 + U_2 = 5 RT + 6 RT = 11 RT$.

$A$ gas mixture consists of $2$ moles of $O_2$ and $4$ moles of $Ar$ at temperature $T$. Neglecting all vibrational modes,the total internal energy of the system is: (in $RT$)

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