What is the mean free path for the molecules in an ideal gas when the pressure is 100 kPa and the temperature is 300 K given that the collision cross-section for the molecules of that gas is 2.0 × 10^-20 m²? 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) 1.1 × 10^-6 m B) 2.1 × 10^-6 m C) 1.7 × 10^-6 m D) 5.3 × 10^-6 m E) 1.5 × 10^-6 m

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The Answer of What is the mean free path for the molecules in an ideal gas when the pressure is 100 kPa and the temperature is 300 K given that the collision cross-section for the molecules of that gas is 2.0 × 10^-20 m²? 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) 1.1 × 10^-6 m B) 2.1 × 10^-6 m C) 1.7 × 10^-6 m D) 5.3 × 10^-6 m E) 1.5 × 10^-6 m

What Is the Mean Free Path for the Molecules in an Ideal