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  Entropy and Free Energy Homework Help - K-12 Grade Level, College Level Chemistry

Introduction of Entropy

Entropy is a thermodynamic property i.e. the measure of a system's thermal energy per unit temperature that is not available for doing valuable work. Perhaps, well known manifestation of entropy is that, following the laws of the thermodynamics, the closed system's entropy at all times increases and in heat transfer situations, the heat energy is transferred to lower temperature components from higher temperature components. In thermally isolated systems, entropy runs in only 1 direction. One can measures the entropy of a system to conclude the energy that is unavailable for work in a thermodynamic process, like energy machines, engines, or conversion. This type of devices and processes can only be driven by convertible energy and have a theoretical maximum efficiency while converting energy to work. Throughout this work the entropy accumulates in the system, which then dissipates in form of waste heat.

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In typical thermodynamics, the theory of entropy is described phenomenologically by the 2nd law of thermodynamics, which states that entropy of an isolated system at all the times gets increased or remains constant. So entropy is also a measure of a process's tendency, like a chemical reaction, to be entropically favored or to continue in a specific direction. It determines that the thermal energy at all the time flows spontaneously to regions of lower temperature from regions of higher temperature, in the form of heat. This process reduces the state of order of the initial systems and so entropy is an expression of randomness or disorder. This is the basis of modern microscopic interpretation of entropy in statistical mechanics, where entropy is described as the amount of additional information needed to specify exact physical state of the system, given its thermodynamic specification.

Free energy

In thermodynamics the Free energy, is energy-like state or property function of a system in thermodynamic equilibrium. Free energy has dimensions of energy and its value is defined through the state of the system and not through its history. The Free energy is employed to conclude how systems change and how much work they can produce. It is described into two forms: the Helmholtz free energy F, sometimes known as work function and Gibbs free energy G. If U is internal energy of a system, PV is the pressure-volume product, and TS the temperature-entropy product (T being the temperature above absolute zero), then F = U - TS and G = U + PV - TS. The latter equation can also be written in the form G = H - TS, where H = U + PV is the enthalpy. The Free energy is a wide property that means its magnitude depends on the amount of a substance in a given thermodynamic state.

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