1 / 49

# Entropy - PowerPoint PPT Presentation

Entropy. Time’s Arrow. Objectives. Explain the tendency of matter and energy to spread out over time. Identify entropy changes in familiar processes. Poll Question. I think I know what “entropy” means. True. False. The Flow of Matter. particles disperse. Gas Molecule in a Box.

Related searches for Entropy

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.

## PowerPoint Slideshow about 'Entropy' - paul2

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

### Entropy

Time’s Arrow

• Explain the tendency of matter and energy to spread out over time.

• Identify entropy changes in familiar processes.

I think I know what “entropy” means.

• True.

• False.

### The Flow of Matter

particles disperse

No energy transfer to walls: elastic collisions

Double the size of the box!

Double the size of the box!

a. Allb. Half

c. noned. 75%

Poll Question

What portion of the time will the molecule spend in the original volume (left half of the box)?

What portion of the time will the molecule spend in the original space if we quadruple the volume of the box?

a. Allb. Half

c. 1/3d. 1/4

Poll Question

What portion of the time will the molecule spend in the original space if we quadruple the volume of the box?

a. 1b. 1/2

c. 1/3d. 1/4

Poll Question

What is the probability that the molecule will be in the original space at any given time?

V

V/4

a. 1b. 1/2

c. 1/4d. 0

Two Molecules (Poll)

What is the probability that both will be in the left half of the container at the same time?

a. 1/2b. 1/3

c. 1/4d. 1/8

Three Molecules (Poll)

What is the probability that all three will be in the left half of the container at the same time?

• What is the probability that all N will be in the given sector of the container at the same time?

xV

V

Random motions cause particles to spread out. The chance that they will randomly come back together decreases tremendously as the number of molecules increases.

### The Flow of Energy

energy disperses

A moving object rams a stationary object.

Before impact:Kinetic Energy of projectile > 0 Kinetic Energy of target = 0

What happens to the kinetic energy after the collision?

• All of it goes to the target.

• The projectile and target have equal kinetic energies.

• The projectile keeps it all.

• It depends; there isn’t enough information to know for sure.

I calculated the kinetic energies of object 1 (projectile) and object 2 (target) as a function of

• Offset

• Relative masses

• Before impact, all the kinetic energy is in the motion of the projectile.

• At impact, the kinetic energy almost always distributes to motion of both the projectile and target.

• When two objects collide, their kinetic energies are usually closer after the collision than before.

• Spreads out over more objects

• Spreads out in more directions

• Work becomes internal energy

• How does entropy increase when a ball is dropped, bounces, and eventually stops?

• How is energy conserved?

• Bouncing ball example applet www.chem.uci.edu/undergraduate/applets/bounce/bounce.htm

PEKErandom molecular KE

### Heat Transfer

multiple interactions

Two solids with different temperatures (average molecular kinetic energies) are brought into contact.

Two solids with different temperatures (average molecular kinetic energies) are brought into contact. What happens to the atoms’ kinetic energies (temperatures)?

Molecular kinetic energy flows from high temperature objects to low temperature objects, but not the other way around.

This is because kinetic energy tends to even out between colliding objects.

There are more ways to distribute energy among many molecules than among few molecules.

Hot

Cold

heat

Until

Warm

Warm

Equilibrium

Hot

Heat flows until total entropy stops increasing

• Thermal equilibrium

• Same temperature

Cold

heat

DS

DS

high

low

DU

DU

Hot

1/T = DS/DU

DS = q/T

Cold

heat

DS

DS

high

low

DU

DU

• Particles and energy tend to become spread out uniformly.

• Entropy is a measure of how many different ways a state can be arranged.

• libraryanalogy

• Total entropy increases in all processes that actually occur.

### What It Means

examples

We cannot see most of the motion that occurs in our world.

• How can matter ever become localized?

• Stars form

• Rain falls

• How can thermal motion ever decrease?

• Refrigerators and heat pumps

• First aid cold packs

• Any time one thing becomes localized, something else spreads out more

• W = number of “configurations” of a state

• S = kBln(W) = entropy of the state

• DS = entropy change

• DS = S2− S1

• = kBln(W2) − kBln(W1)

• = kBln(W2/W1)

• W2/W1 =

= xN

N

xV

V

• DS = kNln(x)

xV

V

• Any energy molecular motion

• Raises entropy

• Energy less constrained

• Effect more important at low temperatures

• DS = q/T

• Greater proportional increase in thermal energy at low T

• Solid  liquid

• disperses matter DSc > 0

• constrains energy DST < 0

DSc

DS

DS

0

temp

DST

melting temperature

• Salt dissolves in liquid only

• Raises S of liquid (+ salt)

• Raises DSc

lower melting temperature

DSc

DSc

DS

DS

DS

0

temp

DST

original melting temperature

• How can matter ever become localized?

• Stars form

• Rain falls

• How can temperature ever decrease?

• Refrigerators and heat pumps

• First aid cold packs

• Whenever one thing becomes localized, something else spreads out more

• Could the reverse process occur?

• What spreads out: matter, energy or both? How?

• Why does total entropy increase?

• Enthalpy (DH) is heat transfer to surroundings

• Spontaneous if DG = DH – TDS < 0

• Equivalent to DS – DH/T > 0

• DS is entropy change of system

• DH/T is entropy change of surroundings

• If a state changes spontaneously, entropy increases.

• Darwinian evolution is perfectly consistent with thermodynamics.

• Energy from the sun powers life processes.

• Energy from earth radiates into space.

• Material order on earth can increase because energy is dispersed.

• Entropy always increases!

### Congratulations!

“[Asking someone to] describe the Second law of thermodynamics is about the scientific equivalent of: Have you read a work of Shakespeare’s?”

– C.P. Snow, Rede Lecture, Cambridge, May 7, 1959.