anonymous
  • anonymous
Show me the second law of thermodynamics and example to apply it.
The second law of thermodynamics
  • Stacey Warren - Expert brainly.com
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katieb
  • katieb
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anonymous
  • anonymous
@goformit100
goformit100
  • goformit100
Sure
anonymous
  • anonymous
lets discuss abt it

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RANE
  • RANE
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/seclaw.html this explains wht it is and also provides examples to explain the concept
anonymous
  • anonymous
@RANE, I wanna discuss it here :D cmooon
anonymous
  • anonymous
I've read that @RANE
goformit100
  • goformit100
ya but she wants the explanation. I have many llinks like that ...
anonymous
  • anonymous
LOOOL I give up if you just link me of that lul @goformit100
goformit100
  • goformit100
ok lets start... yu begin first.
anonymous
  • anonymous
btw i just wnna make this subject ALIVE :D
anonymous
  • anonymous
@goformit100 Carnot?
goformit100
  • goformit100
ok
goformit100
  • goformit100
ya do you know 2nd law is defined in about 10 ways by different scientists
anonymous
  • anonymous
nah, tell me 10 :3
anonymous
  • anonymous
suppose Im your student :D
goformit100
  • goformit100
ok
goformit100
  • goformit100
All the spontaneous process are irreversible in nature.
anonymous
  • anonymous
-_-
anonymous
  • anonymous
Why thermodynamics on chem section, not in phys section?
goformit100
  • goformit100
0_0 Open your eyes baby
anonymous
  • anonymous
lol i have small eyes (aka squinty)
goformit100
  • goformit100
That can only be answered by Miss @Preetha
anonymous
  • anonymous
woka woka. im afraid now.
joemc
  • joemc
In chemistry, this is where entropy is usually introduced.....
anonymous
  • anonymous
@joemc . you mean like carnot?
anonymous
  • anonymous
Oh I see.
joemc
  • joemc
The first law introduces internal energy, U. Second law introduces entropy, S
goformit100
  • goformit100
Entropy of the universe always keeps on increasing
joemc
  • joemc
Carnot is brought in here, at least the Carnot efficiency.
anonymous
  • anonymous
Congratss for 50 SS. :3 I give you amed for it :)) you're awesome ★░░░░░░░░░░░████░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░███░██░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░█░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░██░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░██░░░███░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░██░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░░███░░░░░░░░░░░░░░★ ★░░░░░░░░░░░░██░░░░░░██░░░░░░░░░░░░░★ ★░░░░░░░███████░░░░░░░██░░░░░░░░░░░░★ ★░░░░█████░░░░░░░░░░░░░░███░██░░░░░░★ ★░░░██░░░░░████░░░░░░░░░░██████░░░░░★ ★░░░██░░████░░███░░░░░░░░░░░░░██░░░░★ ★░░░██░░░░░░░░███░░░░░░░░░░░░░██░░░░★ ★░░░░██████████░███░░░░░░░░░░░██░░░░★ ★░░░░██░░░░░░░░████░░░░░░░░░░░██░░░░★ ★░░░░███████████░░██░░░░░░░░░░██░░░░★ ★░░░░░░██░░░░░░░████░░░░░██████░░░░░★ ★░░░░░░██████████░██░░░░███░██░░░░░░★ ★░░░░░░░░░██░░░░░████░███░░░░░░░░░░░★ ★░░░░░░░░░█████████████░░░░░░░░░░░░░★ ★░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░★ @joemc BACK TO CHEM
joemc
  • joemc
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
goformit100
  • goformit100
@Machida you care so much of others. you are so kind to the good ones.
anonymous
  • anonymous
@joemc . wait, whats for exactly that law? chem or phys first? Ya, I dont think abt it before. :o
anonymous
  • anonymous
@goformit100 because caring each other for intelligence is awesome :)
joemc
  • joemc
You would calculate the entropy of the system at each temperature and then calculate the difference.... Equation to follow....
anonymous
  • anonymous
wow, im too stupid of that :/
joemc
  • joemc
At constant pressure: \[S(T_F) = S(T_i) + \int\limits_{i}^{f} (\frac{ C_P }{ T })dT\] At constant volume: \[S(T_F) = S(T_i) + \int\limits\limits_{i}^{f} (\frac{ C_V }{ T })dT\]
joemc
  • joemc
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.
joemc
  • joemc
What types of problems are you looking for...the Gibbs function also is part of this and probably more approachable.
anonymous
  • anonymous
Well, let me do it tomorrow. i need to understanding that materials again. :D btw thanks a lot for make me thought abt it
joemc
  • joemc
OK, good night!
anonymous
  • anonymous
Good noon :D
Frostbite
  • Frostbite
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

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