01:160:161 Chapter Notes - Chapter 10.1-10.2: Kinetic Theory Of Gases

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Pressure is the force exerted per unit area by gas particles as they strike surfaces around them. Gaseous atoms or molecules exert a force when they collide with a surface. The result of many of these collisions is pressure- the constant force on the surfaces exposed to any gas. The total pressure exerted by a gas depends on several factors, including the concentration of gas particles in the sample; the lower the concentration, the lower the pressure. According to the kinetic molecular theory of gases, a gas is a collection of particles (either molecules or atoms, depending on the gas) in constant motion. A single particle moves in a straight line until it collides with another partial (or with the wall of the container) The kinetic molecular theory of gases gas three basic postulates (or assumptions): the size of a particle is negligibly small.

Related Questions

Which statement is false?

A.	The molecules of an ideal gas are relatively very far apart on the average.

B.	At a given temperature, according to the kinetic molecular theory, the average velocity of He atoms is the same as the average velocity of F₂ molecules.

C.	The average kinetic energies of molecules of samples of different ideal gases at the same temperature are the same.

D.	The molecules of a gas move in straight paths until they collide with other molecules or the walls of their containers, according to the kinetic molecular theory.

1.) A gas is found to have a density of 3.165 g/L at STP. What is its molar mass? Which of the following gases is it most likely to be?

Molar Mass: _________

a. NH3
b. O2
c. Cl2

d. SF6

2.) Calculate the pressure exerted by 5.05 moles of NCl3 gas in a 20.00-L container at -205Â°C for a real gas. (for xenon: a= 42.63 atmÂ·L2/mol2 and b= 0.2450 L/mol)

3.) Which of the following is NOT true in the kinetic molecular theory of ideal gases?

The size of the molecules are negligible compared to the volume of the container

The kinetic energy of a sample is proportional to the temperature of the gas.

Collisions are elastic (no friction occurs between the molecules when they collide)

The pressure of a sample is affected by which gases are present.

I have reached the surface, but too quickly, so I had to use the dry decompression chamber. In the dry decompression chamber, I had some time to think and imagine. I really thought I saw small gas molecule floating around. Fill-in the postulates of the Kinetic Molecular Theory below.

The Postulates:

I.The total volume in which the gas is contained is mostly _____________ space. The ___________ of the gas is negligible.

II.Gas molecules are in continuous _____________ _____________ in all directions.

III.Energy is _____________ from one molecule to another, but the total energy remains _____________ at a constant temperature.

IV.Molecules of a gas neither_____________ or _____________ each other.

V.The average KE of gas particles depends only on the absolute _____________ of the gas

Nowâ¦ Match each postulate them to the observational statements below by putting the corresponding Roman numeral in front of each statement

1) ______The gas molecules didnât really seem interested in each other

2) ______They never seemed to lose energy, no matter how many times they bumped into each other

3) ______I couldnât believe we could actually breathe, considering there seemed to be so few molecules.

4) ______They even seemed to move faster when they got nearer to me.

5)( ______The molecules seemed to have no rhyme or reason in their movements

01:160:161 Chapter Notes - Chapter 10.1-10.2: Kinetic Theory Of Gases

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