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Machida

  • one year ago

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

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  1. Machida
    • one year ago
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    @goformit100

  2. goformit100
    • one year ago
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    Sure

  3. Machida
    • one year ago
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    lets discuss abt it

  4. RANE
    • one year 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
    • one year ago
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    @RANE, I wanna discuss it here :D cmooon

  6. Machida
    • one year ago
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    I've read that @RANE

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

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

  9. goformit100
    • one year ago
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    ok lets start... yu begin first.

  10. Machida
    • one year ago
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    btw i just wnna make this subject ALIVE :D

  11. Machida
    • one year ago
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    @goformit100 Carnot?

  12. goformit100
    • one year ago
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    ok

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

  14. Machida
    • one year ago
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    nah, tell me 10 :3

  15. Machida
    • one year ago
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    suppose Im your student :D

  16. goformit100
    • one year ago
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    ok

  17. goformit100
    • one year ago
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    All the spontaneous process are irreversible in nature.

  18. Machida
    • one year ago
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    -_-

  19. Machida
    • one year ago
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    Why thermodynamics on chem section, not in phys section?

  20. goformit100
    • one year ago
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    0_0 Open your eyes baby

  21. Machida
    • one year ago
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    lol i have small eyes (aka squinty)

  22. goformit100
    • one year ago
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    That can only be answered by Miss @Preetha

  23. Machida
    • one year ago
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    woka woka. im afraid now.

  24. joemc
    • one year ago
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    In chemistry, this is where entropy is usually introduced.....

  25. Machida
    • one year ago
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    @joemc . you mean like carnot?

  26. Machida
    • one year ago
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    Oh I see.

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

  28. goformit100
    • one year ago
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    Entropy of the universe always keeps on increasing

  29. joemc
    • one year ago
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    Carnot is brought in here, at least the Carnot efficiency.

  30. Machida
    • one year 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
    • one year 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
    • one year ago
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    @Machida you care so much of others. you are so kind to the good ones.

  33. Machida
    • one year 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
    • one year ago
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    @goformit100 because caring each other for intelligence is awesome :)

  35. joemc
    • one year 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
    • one year ago
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    wow, im too stupid of that :/

  37. joemc
    • one year 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
    • one year 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
    • one year 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
    • one year 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
    • one year ago
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    OK, good night!

  42. Machida
    • one year ago
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    Good noon :D

  43. Frostbite
    • one year 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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