Assuming the radius of diatomic molecules is approximately 1.0 × 10^-10m, for what pressure will the mean free path in room-temperature (20°C) nitrogen be 4.6 m? The Boltzmann constant is 1.38 × 10^-23 J/K, Avogadro's number is 6.02 × 10²³ molecules/mole, and the ideal gas constant is R = 8.314 J/mol•K = 0.0821 L ∙ atm/mol ∙ K. A) 4.9 × 10^-8_atm B) 6.9 × 10^-8_atm C) 1.5 × 10^-7_atm D) 2.2 × 10^-7_atm

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Quizplus · Accepted Answer

The mean free path λ is given by λ = (kT)/(√2 * π * d² * P), where k is the Boltzmann constant, T is the temperature in Kelvin, d is the diameter of the molecule, and P is the pressure. Solving for P with the given values, the pressure is approximately 4.9 × 10⁻⁸ atm.

Assuming the Radius of Diatomic Molecules Is Approximately 1