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:

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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: (f 1 +f 2 )/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.

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

Concept context

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