A gas mixture consists of 2 moles of oxygen a | vedclass

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(D) Oxygen is a diatomic gas,so its internal energy for $n_1 = 2$ moles is given by $U_1 = n_1 	imes \frac{f_1}{2} RT$,where $f_1 = 5$ (degrees of fr

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$11$

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(D) Oxygen is a diatomic gas,so its internal energy for $n_1 = 2$ moles is given by $U_1 = n_1 	imes \frac{f_1}{2} RT$,where $f_1 = 5$ (degrees of freedom for diatomic gas).$U_1 = 2 	imes \frac{5}{2} RT = 5 RT$.Argon is a monoatomic gas,so its internal energy for $n_2 = 4$ moles is given by $U_2 = n_2 	imes \frac{f_2}{2} RT$,where $f_2 = 3$ (degrees of freedom for monoatomic gas).$U_2 = 4 	imes \frac{3}{2} RT = 6 RT$.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 oxygen and $4$ moles of argon at temperature $T$. Neglecting all vibrational modes,the total internal energy of the system is: (in $RT$)

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