of+Gases

= Kinetic-Molecular Theory of Gases: A model for ideal gases. = //ideal gas// - a hypothetical gas that fits all of the assumptions of the Kinetic-Molecular Theory of Gases

Assumptions of the Kinetic-Molecular Theory of Gases
// The five assumptions of the Kinetic-Molecular Theory of Gases are listed below. With a partner you will contribute to class explanations of each assumptions. Please remember to give credit to your sources. Also, please make your contributions in black-font. //

//1. "Gases that consist of large numbers of tiny particles that are far apart relative to their size."//
How does the volume of a certain number of particles of a gas compare to the volume of the same number of particles of a liquid or gas?

Explain how the density of a gas compare to that of a solid or a liquid.

//gas compression// -

//elastic collisions// -

Anything in motion has kinetic energy, so how does the kinetic energy of each particle of an ideal gas change when two collide? How does the total kinetic energy of both particles change?

//3. "Gas particles are in continuous, rapid, random motion. They therefore possess kinetic energy, which is energy of motion."//
The kinetic energy of gases allow them to overcome what force?

The exception is when the gas particles are at the temperature where they condense to form a liquid or solid. At this temperature, the particles become attracted to one another.

Why is it that there are no forces of attraction between gas particles?

The formula for kinetic energy is:

The symbols in this equation represent: KE = kinetic energy m = v =

A higher kinetic energy results in a (higher/lower)temperature.

A lower kinetic energy results in a (higher/lower)temperature.

Faster moving gas particles result in a (higher/lower)temperature.

Slower moving gas particles result in a (higher/lower)temperature.

Considering the following statement and the mass of each gas, what would the speed of nitrogen gas be, compared to the speed of oxygen gas, if both gases had the same temperature?

“All gases at the same temperature have the same average kinetic energy.”

Recommended resources: a physics book

// Explained by the Assumptions of the Kinetic-Molecular Theory of Gases. //
// Though, ideal gases do not exist, many gases behave very much like an ideal gas if the temperature is not too low nor the pressure too high. Many of the characteristics of real gases can be explained by the assumptions of the Kinetic-Molecular Theory of Gases. For tonight's assignment, you are to identify and explain which assumption accounts for the physical properties of gases. //


 * Follow the link to access the document for this assignment: [|Assignment]**

EXPANSION
Gases do not have a definite shape or volume, but expand to completely fill any container in which they are enclosed.

Assumption(s):

FLUIDITY
Particles glide easily past one another. In other words they flow, like liquids do. Both liquids and gases are considered fluids because they flow.

Assumption(s):

**LOW DENSITY**
Gases have a very low density compared to the density of solids and liquids. In comparison, gas density is nearly 1/1000 that of solid or liquid density.

Assumptions(s):

COMPRESSIBILITY
The volume of a sample of gas can be greatly changed. It can be compressed to a much smaller volume, creating a greater pressure.

Assumption(s):

diffusion - spontaneous mixing of the particles of two substances caused by their random motion effusion - a process by which gas particles pass through a tiny opening

Assumption(s):

// Reference: The 1st section of the 10th chapter of HOLT Modern Chemistry (2006). //

ICC Standard:
Science: Physical Science Understand and apply knowledge of the structure and properties of matter.

MISIC Benchmark:
S.09-12.CH.04.08: Benchmark: Compares and contrasts solids, liquids and gases and their changes in state. Description: The student will understand the difference in solids, liquids, and gases due to distances and angles between the molecules or atoms.