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anonymous
 3 years ago
Show me the second law of thermodynamics and example to apply it.
anonymous
 3 years ago
Show me the second law of thermodynamics and example to apply it.

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RANE
 3 years ago
Best ResponseYou've already chosen the best response.0http://hyperphysics.phyastr.gsu.edu/hbase/thermo/seclaw.html this explains wht it is and also provides examples to explain the concept

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0@RANE, I wanna discuss it here :D cmooon

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1ya but she wants the explanation. I have many llinks like that ...

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0LOOOL I give up if you just link me of that lul @goformit100

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1ok lets start... yu begin first.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0btw i just wnna make this subject ALIVE :D

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1ya do you know 2nd law is defined in about 10 ways by different scientists

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0suppose Im your student :D

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1All the spontaneous process are irreversible in nature.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0Why thermodynamics on chem section, not in phys section?

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.10_0 Open your eyes baby

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0lol i have small eyes (aka squinty)

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1That can only be answered by Miss @Preetha

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0woka woka. im afraid now.

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1In chemistry, this is where entropy is usually introduced.....

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0@joemc . you mean like carnot?

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1The first law introduces internal energy, U. Second law introduces entropy, S

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.1Entropy of the universe always keeps on increasing

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1Carnot is brought in here, at least the Carnot efficiency.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0Congratss for 50 SS. :3 I give you amed for it :)) you're awesome ★░░░░░░░░░░░████░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░███░██░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░█░░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░██░░░██░░░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░██░░░███░░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░██░░░░░░░░░░░░░░░░★ ★░░░░░░░░░░░██░░░░░███░░░░░░░░░░░░░░★ ★░░░░░░░░░░░░██░░░░░░██░░░░░░░░░░░░░★ ★░░░░░░░███████░░░░░░░██░░░░░░░░░░░░★ ★░░░░█████░░░░░░░░░░░░░░███░██░░░░░░★ ★░░░██░░░░░████░░░░░░░░░░██████░░░░░★ ★░░░██░░████░░███░░░░░░░░░░░░░██░░░░★ ★░░░██░░░░░░░░███░░░░░░░░░░░░░██░░░░★ ★░░░░██████████░███░░░░░░░░░░░██░░░░★ ★░░░░██░░░░░░░░████░░░░░░░░░░░██░░░░★ ★░░░░███████████░░██░░░░░░░░░░██░░░░★ ★░░░░░░██░░░░░░░████░░░░░██████░░░░░★ ★░░░░░░██████████░██░░░░███░██░░░░░░★ ★░░░░░░░░░██░░░░░████░███░░░░░░░░░░░★ ★░░░░░░░░░█████████████░░░░░░░░░░░░░★ ★░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░░★ @joemc BACK TO CHEM

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1But, 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
 3 years ago
Best ResponseYou've already chosen the best response.1@Machida you care so much of others. you are so kind to the good ones.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0@joemc . wait, whats for exactly that law? chem or phys first? Ya, I dont think abt it before. :o

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0@goformit100 because caring each other for intelligence is awesome :)

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1You would calculate the entropy of the system at each temperature and then calculate the difference.... Equation to follow....

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0wow, im too stupid of that :/

joemc
 3 years ago
Best ResponseYou've already chosen the best response.1At 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
 3 years ago
Best ResponseYou've already chosen the best response.1So, 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
 3 years ago
Best ResponseYou've already chosen the best response.1What types of problems are you looking for...the Gibbs function also is part of this and probably more approachable.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0Well, let me do it tomorrow. i need to understanding that materials again. :D btw thanks a lot for make me thought abt it

Frostbite
 3 years ago
Best ResponseYou've already chosen the best response.1I 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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