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1. Potential energy is the energy of attraction/repulsion between "things", they can be atoms/electrons etc. While Potential energy can be used to calculate Free Energy, which, in your context is the WORK required to form a molecule, Potential energy is not the same as Free energy. I would start here: understand what Free Energy is, for ...
Form a C−S C − S bond of acetyl-CoA. This means that the enthalpy of formation: ΔH = (346 + 363) − (799 + 272) =−362 kJ/mol Δ H = (346 + 363) − (799 + 272) = − 362 k J / m o l. That is, this reaction releases 362 kJ/mol 362 k J / m o l worth of energy. The best way to think about bond energies, is to consider that the "bond energy ...
The dimensions are energy per amount of substance (with units of e.g. J/mol). The term "Gibbs energy" is used for a lot of things, and the dimensions could be energy, or energy per amount of substance. The Gibbs energy of reaction $\Delta_r G$, arguably the most important Gibbs energy for a chemist, is defined as:
You can certainly turn electromagnetic energy into chemical energy, but the key is 'efficiently.'. A photo-voltaic cell can be used to split water into Hydrogen and Oxygen. The Hydrogen can be burned or used in a fuel cell. But the key is how efficient is 'efficient.'. Each step will lose energy, but if solar is the input, there is a huge supply.
Then for the second statement, energy is released when bonds are formed. When the PE of the reactants is greater than the PE of the products, heat is released and we have an exothermic process. Consider the conversion of ethane to ethene. This is an endothermic reaction requiring approximately 220 kJ/mol of energy (bonds broken (2X C-H) - bonds ...
N.B.: The term "internal" refers to energy internal to the system. For example, the internal kinetic energy is the energy the system has as a consequence of the thermal motion of its atoms and molecules, as contrasted with the external kinetic energy the system might have as a result of the motion of the system as a whole through space.
The key to understanding how is the relative amount of energy in different chemicals. Some chemical reactions release heat because the products of the reaction are lower energy than the chemicals that react (reactions are a bit more complicated than this in reality and some are driven by changes in entropy but that isn't important for ...
Before the reaction takes place the system of HX2 H X 2 and OX2 O X 2 molecules are in a metastable state: Given enough energy > activation energy the system gains enough energy to overcome the potential barrier and falls into a state of lower energy than the initial state. Share.
Breaking a bond is endothermic. So the inverse is exothermic. Energy is released when a bond is formed. Apparently you want to just discuss what is happening when an electron approaches a proton from far away (x1 in your drawing) to a shorter distance (x2). The electron is supposed to have no kinetic energy at the beginning, in x1.
2. Three ways to turn chemically stored energy into electricity: a fuel cell: While that works fine for hydrogen or methanol, I'm not sure if sugars are possible, and general "food" won't work. Of course you can chemically convert food into hydrogen or alcohol, or into sth. very specially designed to power a bio fuel cell.