When we study photochemical processes in the upper atmosphere, we need to know how frequently atoms and molecules collide. At an altitude of 20 km, T = 217 K and PN2 = 0.050 atm (for this problem, assume only nitrogen molecules are present). What is the mean free path of N2 at an altitude of km? ( = 0.43 nm2)

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Q: A mixture of CO₂ and Kr weighs 29.6 g and exerts a pressure of 0.895 atm in its container. Since Kr…

A: Given Weight of mixture = 29.6 g Total pressure = 0.895 Pressure due to Kr = 0.295 atm

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A: Kinetic molecular theory gives theoretical background for the rate of reactions.

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Q: At what pressure will the mean free path in room-temperature (20∘C)(20∘C) nitrogen be 1.3 mm ?

A: Mean Free Path is the average distance traveled by a moving molecule between collisions. N2 is a…

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Q: 5.) Calculate the most probable speed of an argon gas (39.95 g/mol) at 298K. A. 1.36 x 103 cm/s B.…

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Q: When we study photochemical processes in the upper atmosphere, we need to know how frequently atoms…

A:

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.