Note 2 - Note 2. Energy 2.1 Ideal gases: A simple system to...

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

View Full Document Right Arrow Icon
1 Note 2. Energy 2.1 Ideal gases: A simple system to play with Ideal gases are a natural place to start learning about thermodynamics. We have some intuition about how gases work and an “ideal” gas is the simplest model. In particular, an ideal gas is a great model system to learn and test our understanding of thermodynamics since all of the fundamental thermodynamic properties we will talk about can be found in them and they allow us to study thermodynamics without getting lost in too much math. Later on, we will study more realistic gases and see the nature of the differences. 2.1.1 Basic properties Like many types of matter, we characterize an ideal gas by certain properties: volume ( V ), pressure ( P ), temperature ( T ), and how many moles of atoms are in the gas ( n ). There is a simple expression relating these quantities: PV = nRT This equation is called the equation of state for this system, since it relates the state variables ( P , n , V , and T ) in this case. Actually, many gases behave like ideal gases in certain conditions (this is called “ideal” conditions). R is called the gas constant R and R = 8.314 J/(mol K) 0.082 L atm/(mol K) You will learn later that R is related to the Boltzmann constant, k (=1.38 × 10 -23 J/K) and the Avogadro number N A (=6.02 × 10 -23 /mol) by R = k N A This equation also tells that you need only two variables (two out of P, V and T) to define the state of a gas (with a fixed n). This is true not just for ideal gas but also for any gas system. There are two types of properties here: 1. Extensive properties are properties which are related to “how much stuff” there is. For example, n and V are extensive properties. If the system is duplicated, these variables get doubled. 2. Intensive properties are independent of the size of the system. For example, P , T , are intensive properties. So is the density ρ = N/V , where N is the total number of atoms.
Background image of page 1

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

View Full DocumentRight Arrow Icon
2 2.1.2 A brief glimpse of phase transitions: Van der Waals equation When gases cool, they condense to liquids. When liquids cool, they freeze into solids. These are two examples of phase transitions. However, ideal gases cannot have phase transitions. This is what is meant by “ideal.” Thus, far from the phase transition, they are good models, but do not work well near the phase transition. What makes a phase transition? Interaction between molecules. Gas particles start to stick together at lower temperatures and form a liquid. How can we model this interaction? We can modify the ideal gas equation to include interactions. We’ll do so in two steps: 1. What’s the probability that a gas particle will bump into another one? The density ρ = N/V is a lot like a probability that we’ll find a given particle at a given spot. If the density is high, then there is a high probability that the particle is there. The probability of finding two particles at the same spot goes like the 2 . It’s like what’s the probability of flipping two coins and having them both come up heads: it’s the probability of one coming up heads squared.
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 05/04/2010 for the course CH 43445 taught by Professor Lim during the Spring '10 term at University of Texas at Austin.

Page1 / 16

Note 2 - Note 2. Energy 2.1 Ideal gases: A simple system to...

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