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Home » A gas mixture consists of 2.0 moles of oxygen and 4.0 moles of neon a temperature T. Neglecting all vibrational modes, calculate the total internal energy of the system. (Oxygen has two rotational modes.)
A gas mixture consists of 2.0 moles of oxygen and 4.0 moles of neon a temperature T. Neglecting all vibrational modes, calculate the total internal energy of the system. (Oxygen has two rotational modes.)
CBSE | Class 11 | Kinetic Theory | NCERT Exemplar | Physics
A gas mixture consists of 2.0 moles of oxygen and 4.0 moles of neon a temperature T. Neglecting all vibrational modes, calculate the total internal energy of the system. (Oxygen has two rotational modes.)

Answer:

We know that oxygen has 5 degrees of freedom. Therefore, energy per mole = (5/2)RT

Therefore, for 2 moles of oxygen, energy = 5RT

Neon has 3 degrees of freedom. Therefore, energy per mole for neon = (3/2)RT

For 4 mole of neon, we can write the expression for energy

= 4 x (3/2) RT

= 6RT

Therefore, the total energy = 11RT

 

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