Understanding why enthalpy can be viewed as "heat content" in a constant pressure system. Created by Sal Khan. Watch the next lesson: https://www.khanacademy.

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The enthalpy change for the following reaction is -137 kJ. Using bond energies, estimate the C-C bond energy in C2H6(g). I need a correct answer please thank you. and if you can, properly explain how.

The standard enthalpy of formation is measured in units of energy per amount of substance, usually stated in kilojoule per mole (kj mol 1), but also in kilocalorie per mole, joule per mole or kilocalorie per gram (any combination of these units conforming to the energy per mass or amount guideline).

enthalpy – (thermodynamics) a thermodynamic quantity equal to the internal energy of a system plus the product of its volume and pressure; "enthalpy is the amount of energy in a system capable of doing mechanical work" heat content, total heat, H physical property – any property used to characterize matter and energy and their interactions

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Enthalpy tells us the total energy of a system and how much heat it uses at constant pressure. Mathematically, enthalpy is the sum of the internal energy of a system and the work done by or to that system. Work is the product of the system’s pressure and volume. The units of enthalpy are the same as the units of.

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The key difference between enthalpy and entropy is that enthalpy is the heat transfer taking place in a constant pressure whereas entropy gives an idea of the randomness of a system.. For the study purposes in chemistry, we divide the universe into two as a system and surrounding. At any time, the part we are going to study is the system, and the rest is surrounding.

{eq}\Delta H^\circ_{rxn} = \sum n \Delta H^\circ_{products} – \sum n \Delta H^\circ_{reactants} {/eq}, where n is the number of moles. The values of the {eq}H^\circ.