Kinetic Molecular Theory (KMT) claims that a gas is composed of molecules that move at a constant and also random rate. The collisions in between molecules are perfectly elastic so that no energy is wasted.

The molecules relocate in straight lines until they collide

Energy because this activity is expressed as Kinetic energy (KE) which have the right to be formulated as:

The average kinetic energy value is only affected by temperature changes. The better the temperature, the average kinetic energy of the molecule increases

This molecule is very little once compared to the distance between molecules, so the volume of gas contains mostly empty space

Gas pwrite-ups move randomly (both speed and also direction , as vector)

Average velocities of gases can be expressed as root-mean-square averperiods. (V rms)

R = gas consistent, T = temperature, Mm = molar mass of the gas particles

From the question

R= 8.314 J/mol K

T = 29 + 273 = 302 K

Mm = molar mass O₂ = 2.16 = 32 g/mol = 32.10-3 kg/mol

Discover moreinertia impact in the time of a collision

Henry"s Law

right gas

Keywords: Kinetic Molecular Theory, Collisions, The average kinetic power, the rms speed, gas molecule

You are watching: Calculate the rms speed of an oxygen gas molecule, o2, at 21.0 ∘c .

The μ rms rate = 475,433 m / s

Further explanationGas pwrite-ups move randomly (both speed and also direction, as vector)

Typical velocities of gases have the right to be expressed as root-mean-square velocity. (μ rms)

R = gas continuous, 8,314 J / mol K

T = temperature,K

Mm = molar mass of the gas pposts, Kg

μ rms = root intend square velocity of Gas Particles.,m/s

From this equation reflects that the velocity of the gas is inversely proportional to the molar mass of the gas particles

μ ≅ 1 / Mm

So that the greater the molar mass of the gas pposts, the smaller the speed (the slowest)

Oxygen gas molecule, O₂ has a molar mass: 0.032 kg / mol

T = 17 °C = 17 + 273 = 290 K

then:

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The gas pshort article that travels the slowest

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The μ rms rate = 489.9661 m / s

Further explanationGas pshort articles relocate randomly (both speed and direction, as vector)

Typical velocities of gases have the right to be expressed as root-mean-square velocity. (V rms)

R = gas constant, 8.314 J / mol K

T = temperature,

Mm = molar mass of the gas particles

μ rms = root mean square velocity of Gas Pshort articles.

From this equation mirrors that the velocity of the gas is inversely proportional to the molar mass of the gas particles

μ ≅ 1 / mm

So that the higher the molar mass of the gas pwrite-ups, the smaller the speed (the slowest)