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Machida

  • 2 years ago

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

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  1. Machida
    • 2 years ago
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    @goformit100

  2. goformit100
    • 2 years ago
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    Sure

  3. Machida
    • 2 years ago
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    lets discuss abt it

  4. RANE
    • 2 years ago
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    http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/seclaw.html this explains wht it is and also provides examples to explain the concept

  5. Machida
    • 2 years ago
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    @RANE, I wanna discuss it here :D cmooon

  6. Machida
    • 2 years ago
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    I've read that @RANE

  7. goformit100
    • 2 years ago
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    ya but she wants the explanation. I have many llinks like that ...

  8. Machida
    • 2 years ago
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    LOOOL I give up if you just link me of that lul @goformit100

  9. goformit100
    • 2 years ago
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    ok lets start... yu begin first.

  10. Machida
    • 2 years ago
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    btw i just wnna make this subject ALIVE :D

  11. Machida
    • 2 years ago
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    @goformit100 Carnot?

  12. goformit100
    • 2 years ago
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    ok

  13. goformit100
    • 2 years ago
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    ya do you know 2nd law is defined in about 10 ways by different scientists

  14. Machida
    • 2 years ago
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    nah, tell me 10 :3

  15. Machida
    • 2 years ago
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    suppose Im your student :D

  16. goformit100
    • 2 years ago
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    ok

  17. goformit100
    • 2 years ago
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    All the spontaneous process are irreversible in nature.

  18. Machida
    • 2 years ago
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    -_-

  19. Machida
    • 2 years ago
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    Why thermodynamics on chem section, not in phys section?

  20. goformit100
    • 2 years ago
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    0_0 Open your eyes baby

  21. Machida
    • 2 years ago
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    lol i have small eyes (aka squinty)

  22. goformit100
    • 2 years ago
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    That can only be answered by Miss @Preetha

  23. Machida
    • 2 years ago
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    woka woka. im afraid now.

  24. joemc
    • 2 years ago
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    In chemistry, this is where entropy is usually introduced.....

  25. Machida
    • 2 years ago
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    @joemc . you mean like carnot?

  26. Machida
    • 2 years ago
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    Oh I see.

  27. joemc
    • 2 years ago
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    The first law introduces internal energy, U. Second law introduces entropy, S

  28. goformit100
    • 2 years ago
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    Entropy of the universe always keeps on increasing

  29. joemc
    • 2 years ago
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    Carnot is brought in here, at least the Carnot efficiency.

  30. Machida
    • 2 years ago
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    Congratss for 50 SS. :3 I give you amed for it :)) you're awesome ★░░░░░░░░░░░████░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░███░██░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░█░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░██░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░██░░░███░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░██░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░░███░░░░░░░░░░░░░░★ ★░░░░░░░░░░░░██░░░░░░██░░░░░░░░░░░░░★ ★░░░░░░░███████░░░░░░░██░░░░░░░░░░░░★ ★░░░░█████░░░░░░░░░░░░░░███░██░░░░░░★ ★░░░██░░░░░████░░░░░░░░░░██████░░░░░★ ★░░░██░░████░░███░░░░░░░░░░░░░██░░░░★ ★░░░██░░░░░░░░███░░░░░░░░░░░░░██░░░░★ ★░░░░██████████░███░░░░░░░░░░░██░░░░★ ★░░░░██░░░░░░░░████░░░░░░░░░░░██░░░░★ ★░░░░███████████░░██░░░░░░░░░░██░░░░★ ★░░░░░░██░░░░░░░████░░░░░██████░░░░░★ ★░░░░░░██████████░██░░░░███░██░░░░░░★ ★░░░░░░░░░██░░░░░████░███░░░░░░░░░░░★ ★░░░░░░░░░█████████████░░░░░░░░░░░░░★ ★░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░★ @joemc BACK TO CHEM

  31. joemc
    • 2 years ago
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    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

  32. goformit100
    • 2 years ago
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    @Machida you care so much of others. you are so kind to the good ones.

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

  34. Machida
    • 2 years ago
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    @goformit100 because caring each other for intelligence is awesome :)

  35. joemc
    • 2 years ago
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    You would calculate the entropy of the system at each temperature and then calculate the difference.... Equation to follow....

  36. Machida
    • 2 years ago
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    wow, im too stupid of that :/

  37. joemc
    • 2 years ago
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    At constant pressure: \[S(T_F) = S(T_i) + \int\limits_{i}^{f} (\frac{ C_P }{ T })dT\] At constant volume: \[S(T_F) = S(T_i) + \int\limits\limits_{i}^{f} (\frac{ C_V }{ T })dT\]

  38. joemc
    • 2 years ago
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    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.

  39. joemc
    • 2 years ago
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    What types of problems are you looking for...the Gibbs function also is part of this and probably more approachable.

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

  41. joemc
    • 2 years ago
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    OK, good night!

  42. Machida
    • 2 years ago
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    Good noon :D

  43. Frostbite
    • 2 years ago
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    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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