Lecture9_Ideal_Gas - EAS 1600 Introduction to Environmental...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
EAS 1600 Introduction to Environmental Sciences Class 10 - Ideal Gas Law, Barometric Law In this class we begin a discussion of atmospheric dynamics and its role in determining the climate. Atmospheric dynamics focuses on the motion of air and the resultant weather and climatic phenomena . In the last section on the energy budget, the First Law of Thermodynamics underpinned our discussion. In this section we call on: (i) the kinetic theory of gases ; and (ii) Newton’s Second Law (i. e., F = ma). Today we will begin by showing why we need to worry about atmospheric dynamics’ role in the climate , and then we will review some basic concepts about the nature of a gas and the properties of atmospheric gases under the influence of a gravitational field. We need to consider dynamics because -- An inspection of the radiative energy balance of the earth as a function of latitude indicates an imbalance. There is an energy excess in the tropics and a deficit at high latitudes . Maybe dynamic processes (e.g., winds, etc) move energy from tropics to poles and thus create a balance at all latitudes. ..
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
An ideal gas is -- a gas that obeys the ideal gas law which is a mathematical relationship that governs the gas’ so-called ‘state variables’: ¾ Temperature ¾ Pressure ¾ Density Temperature ¾ A measure of the amount of internal energy (or heat) a substance contains. ¾ The energy is indicated by the random movement of the molecules that make up the substance. ¾ The more energy contained in a substance, the greater the velocity of the molecules, and in turn the greater the temperature. ¾ Temperature is a macroscopic measure of the average kinetic energy contained in the molecules of a given substance ¾ {Avg KE} = ½ m v avg 2 = k B T ¾ Where v avg = average random molecular velocity k B = Boltzmann’s constant = 1.38 x 10 -23 J/K/molecule m = mass of a molecule of the substance = M
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 04/18/2008 for the course EAS 1600 taught by Professor Jimstjohn during the Spring '08 term at Georgia Tech.

Page1 / 5

Lecture9_Ideal_Gas - EAS 1600 Introduction to Environmental...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online