Question

Show me the second law of thermodynamics and example to apply it.

Answer 1

@goformit100

Answer 2

Sure

Answer 3

lets discuss abt it

Answer 4

http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/seclaw.html

this explains wht it is and also provides examples to explain the concept

Answer 5

@RANE, I wanna discuss it here :D cmooon

Answer 6

I've read that @RANE

Answer 7

ya but she wants the explanation. I have many llinks like that ...

Answer 8

LOOOL
I give up if you just link me of that lul @goformit100

Answer 9

ok lets start... yu begin first.

Answer 10

btw i just wnna make this subject ALIVE :D

Answer 11

@goformit100 Carnot?

Answer 12

ok

Answer 13

ya
do you know 2nd law is defined in about 10 ways by different scientists

Answer 14

nah, tell me 10 :3

Answer 15

suppose Im your student :D

Answer 16

ok

Answer 17

All the spontaneous process are irreversible in nature.

Answer 18

-_-

Answer 19

Why thermodynamics on chem section, not in phys section?

Answer 20

0_0 Open your eyes baby

Answer 21

lol i have small eyes (aka squinty)

Answer 22

That can only be answered by Miss @Preetha

Answer 23

woka woka. im afraid now.

Answer 24

In chemistry, this is where entropy is usually introduced.....

Answer 25

@joemc . you mean like carnot?

Answer 26

Oh I see.

Answer 27

The first law introduces internal energy, U. Second law introduces entropy, S

Answer 28

Entropy of the universe always keeps on increasing

Answer 29

Carnot is brought in here, at least the Carnot efficiency.

Answer 30

Congratss for 50 SS. :3 I give you amed for it :)) you're awesome

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@joemc

BACK TO CHEM

Answer 31

But, a second law problem in chemisty could be something like....
Calculate the entropy change when Neon, at 25 C and 1.00 atm in a 500ml container i allowed to expand to 1 L and is simutaneously heated to 100 C

Answer 32

@Machida you care so much of others. you are so kind to the good ones.

Answer 33

@joemc . wait, whats for exactly that law? chem or phys first?
Ya, I dont think abt it before. :o

Answer 34

@goformit100 because caring each other for intelligence is awesome :)

Answer 35

You would calculate the entropy of the system at each temperature and then calculate the difference.... Equation to follow....

Answer 36

wow, im too stupid of that :/

Answer 37

At constant pressure:
\[S(T_F) = S(T_i) + \int\limits_{i}^{f} (\frac{ C_P }{ T })dT\]

At constant volume:
\[S(T_F) = S(T_i) + \int\limits\limits_{i}^{f} (\frac{ C_V }{ T })dT\]

Answer 38

So, you need to break the problem down into two steps and figure the difference of each change. One part is isothermal, the other adiabatic.

Answer 39

What types of problems are you looking for...the Gibbs function also is part of this and probably more approachable.

Answer 40

Well, let me do it tomorrow. i need to understanding that materials again. :D
btw thanks a lot for make me thought abt it

Answer 41

OK, good night!

Answer 42

Good noon :D

Answer 43

I always like to give the following image of the 2. law:
Consider a ball (our system) bouncing of the floor (the surroundings). The ball does not rise as high after each bounce because there are inelastic losses in the materials of the ball and floor. The kinetic energy of the ball’s overall motion is spread out into the energy of thermal motion of its particles and those of the floor that it hits. The direction of spontaneous change is towards a state in which the ball is at rest with all its energy dispersed as the disorderly thermal motion of molecules in the air and spread over the atoms of the virtually infinite floor.

So what are we trying to say:
We look for the direction of change that leads to the random dispersal of the total energy of the isolated system.

Leading to our understanding of the second law of thermodynamics:
The entropy of an isolated system increases in the course of a spontaneous change: ∆S_total > 0