CHEM.10.B

Previous Next
The student is expected to describe and calculate the relationships among volume, pressure, number of moles, and temperature for an ideal gas; and
1666 TEKS header image

Knowledge and Skills Statement

Science concepts. The student understands the principles of the kinetic molecular theory and ideal gas behavior.

The relationships among different physical laws of gasses are shown below, where kB is the Boltzmann constant, 1.380649 × 10-23 Joules (J) per Kelvin (K).

A labeled formula demonstrating the relationships between the combined, ideal, Charles, Boyle, Gay-Lussac, and Avogadro’s gas laws.
Image URL: https://commons.wikimedia.org/wiki/File:Ideal_gas_law_relationships.svg

a hypothetical gas that is composed of molecules following a few rules: ideal gas molecules do not attract or repel each other and take up no space (have no volume)

describes the behavior of ideal gases at the particle level 

Research

Pester, Patrick. "Gases: Structure, Properties and Facts." BBC Science Focus, (2023). https://www.proquest.com/magazines/gases-structure-properties-facts/docview/2842268168/se-2

Summary:  The ideal gas law combines the other gas laws to create an equation (PV = nRT) for a hypothetical ideal gas, which can be used to determine how gas behaves under different conditions.

Research

Holdmeyer, Dan. (2024). "Compressor Lubrication Fundamentals." Tribology & Lubrication Technology 80, no. 2 (2024): 20-23. https://www.proquest.com/scholarly-journals/compressor-lubrication-fundamentals/docview/2923267909/se-2

Summary:  In a previous article, various compressor designs and how some compressors utilize multiple stages to get to higher pressures were discussed. The authors noted that they needed to cool the air between the stages for efficiency and safety reasons. The author started to explain the relationship between gas pressure, volume and temperature using the various gas laws of Boyle's, Charles' and Gay-Lussac's leading to the Ideal Gas Law: PV=nRT (pressure times volume equals number of molecules times R the gas constant times temperature).