For a gas mixture of monatomic and diatomic molecules with degrees of freedom f 1 and f 2 respectively in equal number of moles, the average degrees of freedom of the mixture is:

⚛️ Physics · Kinetic Theory · NEET & JEE

For a gas mixture of monatomic and diatomic molecules with degrees of freedom f₁ and f₂ respectively in equal number of moles, the average degrees of freedom of the mixture is:

Answer: (f₁+f₂)/2.

A f₁ + f₂
B (f₁+f₂)/2
C f₁ × f₂
D (f₁ - f₂)/2

Correct answer: B. (f₁+f₂)/2

Explanation: For an equimolar mixture, the average degrees of freedom is the simple average of the individual values: (f₁+f₂)/2.

Not all gas molecules move at the same speed - the Maxwell-Boltzmann distribution shows the spread, with the most probable speed v_p slightly less than the average v_avg, which is slightly less than the root-mean-square speed v_rms used in the pressure formula.

Concept context

Kinetic theory of gases connects molecular motion to pressure and temperature, explaining gas laws, specific heats, and molecular speeds.

Read the full Kinetic Theory notes →

For a gas mixture of monatomic and diatomic molecules with degrees of freedom f1 and f2 respectively in equal number of moles, the average degrees of freedom of the mixture is:

Concept context

More Kinetic Theory questions

For a gas mixture of monatomic and diatomic molecules with degrees of freedom f₁ and f₂ respectively in equal number of moles, the average degrees of freedom of the mixture is: