Post by IBDaMann on May 29, 2019 18:00:55 GMT
At any given time in any given closed system there is a certain quantity of energy with the potential to accomplish work while the remainder of the energy is unable to accomplish work and is called the system's entropy.
Energy(T) = Work_Potential_Energy(T) + Entropy(T)
Every time energy changes form per the 1st Law of Thermodynamics, which includes work being accomplished, the quantity of work-potential energy decreases and the system's entropy increases:
Per the 1st Law of Thermodynamics:
Energy(T) = Energy(T+1)
Work_Potential_Energy(T) + Entropy(T) = Work_Potential_Energy(T+1) + Entropy(T+1)
However, per the 2nd Law of Thermodynamics:
Work_Potential_Energy(T) >= Work_Potential_Energy(T+1)
...also colloquially expressed as Entropy(T) <= Entropy(T+1)
Usable energy within a system strictly decreases, often expressed as entropy within a system strictly increases. Usable energy eventually reaches zero and ability to perform work eventually ceases. A perpetual motion machine is not possible.
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The temperature of a body cannot increase without additional energy, ergo increasing the temperature of a body is work, and is calculated as the amount of energy transferred to increase the temperature. The 0th Law of Thermodynamics states that bodies of the same temperature have no potential for work (relative to each other) as neither can increase the temperature of the other. Energy only flows from bodies of higher temperature to bodies of lower temperature because those cases represent potential to perform the work needed to increase the temperature of the body of lower temperature. When that happens, the temperature of the body of higher temperature decreases as it loses the quantity of thermal energy required to perform the work of increasing the temperature of the body of lower temperature.
Per the 1st Law of Thermodynamics:
Energy(Warmer_Body,T) + Energy(Cooler_Body,T) = Energy(Warmer_Body,T+1) + Energy(Cooler_Body,T+1)
Energy(Warmer_Body,T) - Work = Energy(Warmer_Body,T+1)
Energy(Cooler_Body,T) + Work = Energy(Cooler_Body,T+1)
However, per the 2nd Law of Thermodynamics:
Temperature(Warmer_Body,T) > Temperature(Warmer_Body,T+1)
Temperature(Cooler_Body,T) < Temperature(Cooler_Body,T+1)
In some cases temperature is increased because of pressure applied to a body. In such cases the energy used to apply the pressure becomes the work which increases the temperature.
In some cases temperature is increased because of the force of friction (contact force plus acceleration). In such cases the energy used to apply the contact force and the energy creating the acceleration become the work which increases the temperature.
Energy(T) = Work_Potential_Energy(T) + Entropy(T)
Every time energy changes form per the 1st Law of Thermodynamics, which includes work being accomplished, the quantity of work-potential energy decreases and the system's entropy increases:
Per the 1st Law of Thermodynamics:
Energy(T) = Energy(T+1)
Work_Potential_Energy(T) + Entropy(T) = Work_Potential_Energy(T+1) + Entropy(T+1)
However, per the 2nd Law of Thermodynamics:
Work_Potential_Energy(T) >= Work_Potential_Energy(T+1)
...also colloquially expressed as Entropy(T) <= Entropy(T+1)
Usable energy within a system strictly decreases, often expressed as entropy within a system strictly increases. Usable energy eventually reaches zero and ability to perform work eventually ceases. A perpetual motion machine is not possible.
________________________________________
The temperature of a body cannot increase without additional energy, ergo increasing the temperature of a body is work, and is calculated as the amount of energy transferred to increase the temperature. The 0th Law of Thermodynamics states that bodies of the same temperature have no potential for work (relative to each other) as neither can increase the temperature of the other. Energy only flows from bodies of higher temperature to bodies of lower temperature because those cases represent potential to perform the work needed to increase the temperature of the body of lower temperature. When that happens, the temperature of the body of higher temperature decreases as it loses the quantity of thermal energy required to perform the work of increasing the temperature of the body of lower temperature.
Per the 1st Law of Thermodynamics:
Energy(Warmer_Body,T) + Energy(Cooler_Body,T) = Energy(Warmer_Body,T+1) + Energy(Cooler_Body,T+1)
Energy(Warmer_Body,T) - Work = Energy(Warmer_Body,T+1)
Energy(Cooler_Body,T) + Work = Energy(Cooler_Body,T+1)
However, per the 2nd Law of Thermodynamics:
Temperature(Warmer_Body,T) > Temperature(Warmer_Body,T+1)
Temperature(Cooler_Body,T) < Temperature(Cooler_Body,T+1)
In some cases temperature is increased because of pressure applied to a body. In such cases the energy used to apply the pressure becomes the work which increases the temperature.
In some cases temperature is increased because of the force of friction (contact force plus acceleration). In such cases the energy used to apply the contact force and the energy creating the acceleration become the work which increases the temperature.