Enthalpy (H) - a measure of the energy within a system. It is the sum of its internal energy and the product of its pressure and volume. Enthalpy has the units J mol-1 or kJ mol-1, Activation energy - the minimum amount of energy required for a successful reaction, Standard enthalpy change of reaction (∆rHº) - the enthalpy change when reactants form products in quantities given in the balanced chemical equation, under standard conditions and with all species in their standard states, Standard enthalpy change of formation (∆fH°) - the enthalpy change when one mole of a species is formed from its elements, under standard conditions and with all species in their standard states, Standard enthalpy change of combustion (∆cH°) - the enthalpy change when one mole of a substance burns completely in oxygen under standard conditions with all species in their standard states, Standard enthalpy change of neutralisation (∆nH°) - the enthalpy change when an acid solution and an alkali solution react under standard conditions to form one mole of water, Calorimetry - A technique used to measure the heat transfer in a chemical reaction. It is a way of calculating enthalpy change, Enthalpy of atomisation - the enthalpy change when one mole of gaseous atoms is formed from the element in its standard state, under standard conditions, First Ionisation Energy - he enthalpy change when one mole of electrons is removed from one mole of gaseous atoms to form one mole of gaseous ions with a single positive charge, First electron affinity - the enthalpy change when one mole of gaseous atoms gains one mole of electrons to form into one mole of gaseous negative ions,

Year 12 Enthalpy definitions

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