<p>Notes on the Kinetic-Molecular Theory of Gases Name </p><p>The kinetic-molecular theory of gases is based on the idea that </p><p>An ideal gas is </p><p>5 Assumptions of Kinetic-Molecular Theory</p><p>1.</p><p>2.</p><p>3.</p><p>4.</p><p>5.</p><p>Temperature Conversions between Kelvin and degrees Celsius</p><p>K = C = Properties of a Gas</p><p>______- a gas will completely fill any container it is in.</p><p>______- gas particles, which are initially far apart can be crowded close together</p><p>______- will be ~1/1000th the density of a solid or liquid phase</p><p>______- gas particles glide easily past one another </p><p>______- process of spreading out spontaneously to uniformly occupy a space Illustrate and describe Effusion Illustrate and describe Diffusion</p><p>Rate of Diffusion – depends on two main properties of the gas particles; 1) Size or mass of molecules 2) Temperature of molecules </p><p>Lighter and smaller gas particles will diffuse faster than heavier and larger particles.</p><p>______molecules will diffuse faster than ______molecules.</p><p>Ideal Gas vs. Real Gas Ideal gas - completely conforms to the Kinetic-Molecular theory</p><p>Real gas –</p><p>Ideal Gases Real Gases List properties that are special to each!!</p><p>4 Variables used to describe gases</p><p>1) 3)</p><p>2) 4) </p>