User:QuoJar/sandbox

Grayscale colorspaces more precisely define the interpretation of a grayscale image in terms of the relevant characteristics of the light that should be displayed to the user/viewer at each pixel for each possible numeric sample value. An achromatic (colorimetrically-grayscale) colorspace can be mapped to the achromatic channel of a standard colorspace, irrespective of the values of the chromatic channels. Examples include L* of the CIE L*ab and L*uv colorspaces, the linear luminance Y of the CIE XYZ colorspace, or a "Y'" representing almost any nonlinear version of Y obtained by applying a specific gamma compression function to the linear luminance Y.  a grayscale ICC profile since they are determined solely by the   color.org color [profile] FAQ

In chemistry, chemical potential energy  or simply  chemical energy  is form of potential energy; it is the chemical binding energy (a ) that is released when chemical bonds are formed, or must be supplied when chemical bonds are broken. 'Chemical energy can also be used to mean energy that is made available when chemical potential energy is released and converted to other forms. The chemical potential energy in batteries, fuel, or food, for example, are released when these are used in order to provide energy for devices, vehicles, and animals. A common misconception is that chemical energy is released (evolved) when bonds are broken, whereas in fact breaking bonds requires that energy be absorbed and stored in the chemical system. Chemical (potential) energy is not the same as chemical potential.

Energy that can be released (or absorbed) because of a reaction between a set of chemical substances is equal to the difference between the energy content of the products and the reactants, if the initial and final temperatures are the same. This change in energy can be estimated from the bond energies of the various chemical bonds in the reactants and products. It can also be calculated from $$\Delta {U_f^\circ}_{\mathrm {reactants}}$$, the internal energy of formation of the reactant molecules, and $$\Delta {U_f^\circ}_{\mathrm {products}}$$ the internal energy of formation of the product molecules. The internal energy change of a chemical process is equal to the heat exchanged if it is measured under conditions of constant volume and equal initial and final temperature, as in a closed container such as a bomb calorimeter. However, under conditions of constant pressure, as in reactions in vessels open to the atmosphere, the measured heat change is not always equal to the internal energy change, because pressure-volume work also releases or absorbs energy. (The heat change at constant pressure is called the enthalpy change; in this case the enthalpy of reaction, if initial and final temperatures are equal).

Another useful term is the heat of combustion, which is the energy mostly of the weak double bonds of molecular oxygen released due to a combustion reaction and often applied in the study of fuels. Food is similar to hydrocarbon and carbohydrate fuels, and when it is oxidized to carbon dioxide and water, the energy released is analogous to the heat of combustion (though not assessed in the same way as a hydrocarbon fuel — see food energy).

Chemical potential energy is a form of potential energy related to the structural arrangement of atoms or molecules. This arrangement may be the result of chemical bonds within a molecule or otherwise. Chemical energy of a chemical substance can be transformed to other forms of energy by a chemical reaction. As an example, when a fuel is burned the chemical energy of molecular oxygen is converted to thermal energy, and the same is the case with digestion of food metabolized in a biological organism. Green plants transform solar energy to chemical energy (mostly of oxygen) through the process known as photosynthesis, and electrical energy can be converted to chemical energy and vice versa through electrochemical reactions.

The similar term chemical potential is used to indicate the potential of a substance to undergo a change of configuration, be it in the form of a chemical reaction, spatial transport, particle exchange with a reservoir, etc. It is not a form of potential energy itself, but is more closely related to free energy. The confusion in terminology arises from the fact that in other areas of physics not dominated by entropy, all potential energy is available to do useful work and drives the system to spontaneously undergo changes of configuration, and thus there is no distinction between "free" and "non-free" potential energy (hence the one word "potential"). However, in systems of large entropy such as chemical systems, the total amount of energy present (and conserved by the first law of thermodynamics) of which this Chemical Potential Energy is a part, is separated from the amount of that energy—Thermodynamic Free Energy (which Chemical potential is derived from)—which (appears to) drive the system forward spontaneously as its entropy increases (in accordance with the second law).