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Saturday, November 17, 2012
MECHANICAL ENGINEERING: Thermodynamics - Entropy and the Second Law of Thermodynamics
Entropy
- a measure of a system's energy that is unavailable for work
- a measure of the disorder or randomness
- from Greek entropia "a turning towards"
Second law of thermodynamics
- there is no machine with 100% efficiency
- phenomenon of irreversibility in nature
- In a system, a process that occurs will tend to increase the total entropy of the universe
- The entropy of an isolated system which is not in equilibrium will tend to increase over time, approaching a maximum value at equilibrium
- It is impossible for heat to flow from a colder body to a warmer body without any work having been done to accomplish this flow
- It is impossible to extract an amount of heat from a hot reservoir and use it all to do work. Some amount of heat must be exhausted to a cold reservoir
Few examples of Entropy and the 2nd Law of Thermodynamics
- flow of heat from a hot object to a cold object
- flow of a gas from high pressure to low pressure
- evaporation of water
- melting of ice
- cloud formation in the sky
- adding sugar to a cup of coffee
- carbon dioxide is dissolved in water
- spontaneous (natural) cleaning of a messy house
- shuffling of playing cards
- breaking a mirror or glass
1. Isothermal and reversible process
dS = Q/T
where:
dS = change in entropy, values can be (+)increase or (-)decrease
Q = heat, negative (-) if heat removal, positive (+) if heat addition
T = absolute temperature
2. Temperature not constant
dS = Integral (dQ/T)
dQ = m * c * dT
substituting,
dS = Integral (dQ/T)
dS = Integral (m * c * dT/T)
dS = m * c * Integral (dT/T)
if
T1 = initial temperature
T2 = final temperature
dS = m * c * Integral(T1,T2) (dT/T)
then
dS = m * c * ln T2/T1
where:
m = mass
c = specific heat
dS = change in entropy, values can be (+)increase or (-)decrease
dQ = heat, negative (-) if heat removal, positive (+) if heat addition
T = absolute temperature
1. Find the change in entropy if 1 kg of water at 20 C is changed into ice at 0 C.
find:
dS = total change in entropy
given:
m = 1 kg of water
c of water = 4.2 kJ/kg K
lf = heat of fusion of ice = 334 kJ/kg
T1 = 20 C + 273 = 293 K
T2 = 0 C + 273 = 273 K
solution:
dS = dS1 + dS2
dS1 --> cooling of water
dS1 = m * c * ln T2/T1
dS1 = 1 * 4.2 * ln 273/293
dS1 = - 0.3 kJ/K
dS2 --> freezing of water to ice
dS2 = Q/T
but
Q = - m * lf --> latent heat
note: Q is negative (-) because of HEAT REMOVAL
substituting,
dS2 = - m * lf/T
dS2 = - 1 * 334/273
dS2 = - 1.22 kj/K
total change in entropy
dS = dS1 + dS2
dS = (- 0.3) + (- 1.22)
dS = - 1.52 kJ/K
2. Calculate the change in entropy when 4 kJ of heat flows from the warm exterior at 40 C into a house at 22 C.
find:
dS = total change in entropy
given:
Q = 4 kJ
T exterior = 40 C + 273 = 313 K
T house = 22 C + 273 = 295 K
solution:
dS = dS exterior + dS house
dS exterior:
The entropy of the exterior decreases, since heat flows out of it (- Q)
dS exterior = -Q/T exterior
dS exterior = -4/313
dS exterior = -0.013 kJ/K
dS house:
The entropy of the house increases since heat flows into it (+ Q)
dS house = Q/T house
dS house = 4/295
dS house = 0.014 kJ/K
total change in entropy
dS = dS exterior + dS house
ds = -0.013 + 0.014
dS = 0.001 kJ/K
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