| dQ |
 |
| T |
Entropy is in some sense a measure of disorder.
The symbol for entropy is S, and the units are J/K.
A container of ideal gas has an entropy value, just as it has a pressure, a volume, and a temperature. Unlike P, V, and T, which are quite easy to measure, the entropy of a system is difficult to calculate.
On the other, a change in entropy is easy to determine.
Entropy changes whenever there is a transfer of heat. The change in entropy is the heat added divided by the temperature at which the transfer took place. Expressed as an integral:
| ΔS = Sf - Si | = | ∫ |
|
If the heat transfer takes place at a single temperature, the change in entropy is simply:
| isothermal process: ΔS | = |
|
If the heat transfer takes place over a range of temperatures then, as long as ΔT is small compared to the absolute temperature T, the change in entropy is approximately:
| ΔS | = |
|
For an ideal gas, it can be shown that the change in entropy is given by:
| ΔS | = nR ln | ( |
|
) | + n CV ln | ( |
|
) |
If you spill a glass of milk, what the glass and the milk droplets do is governed by the laws of physics. If you videotaped the spill and then played the film backwards, it would be obvious to you that the film was running backwards. Even though Newton's Laws and The Laws of Conservation of Energy and Conservation of Momentum would be obeyed when you played the film backwards, the probability that all the milk and the glass would spontaneously come together to form a full glass of milk is incredibly small.
This is an example of an irreversible process. The entropy postulate connects the concept of entropy with such processes:
Entropy Postulate: If an irreversible process occurs in a closed system, the entropy S of the system always increases. A reversible process is one in which the system and the surroundings can be returned to the state they were in before the process began. A process is irreversible if energy is lost to friction, or if energy is lost as heat flows from a hot region to a cooler region.
Some processes are reversible. In these there is no change in entropy in a closed system.
The Second Law of Thermodynamics states that:
The entropy of a closed system is constant for reversible processes and increases for irreversible processes. It never decreases.
ΔS ≥ 0
This is why the glass of spilled milk never spontaneously transforms itself back into an upright full glass of milk - that would decrease the entropy.
Entropy is often called time's arrow. Time moves in the direction of increasing entropy.
You have two styrofoam containers of water. Each holds 1 kg of water. In one the water temperature is 17°C, while in the other it is 37°C. The colder water is then poured into the warmer water, and the system is allowed to come to equilibrium.
Assuming no heat is exchanged with the surroundings or the environment, what is the change in entropy in the mixing process?
First, determine how much heat is involved. The final temperature will be 27°C. The heat transferred from the hot water to the cold water is therefore:
Q = mcΔT
m = 1, c = 4186, and ΔT = 10°.
Q = 41860 J
Calculate the change in entropy for the hot and cold water using the equation:
| ΔS | = |
|
The T's are in kelvin. For the cold water, Tavg = 22°C = 295 K. For the hot water Tavg = 32°C = 305 K.
Q is positive for the cold water, because heat was added, and negative for the hot water. Therefore, for the mixing process:
| ΔScold + ΔShot | = |
|
- |
|
= +4.65 J/K |