exothermic reaction, heat energy is released during a reaction, endothermic reaction, heat energy is absorbed during a reaction, enthalpy change, the heat energy transferred during a chemical reaction., activation energy, the minimum energy that colliding particles must possess to break bonds to start a chemical reaction, standard conditions, a pressure of 101 kPa and temperature of 298 K, standard enthalpy change of reaction, the enthalpy change when the amounts of reactants shown in the stoichiometric equation react to give products under standard conditions, standard enthalpy change of formation, the enthalpy change when one mole of a compound is formed from its elements under standard conditions, standard enthalpy change of combustion, the enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions, standard enthalpy change of neutralisation, the enthalpy change when one mole of water is formed by the reaction of an acid with an alkali under standard conditions, specific heat capacity, the energy needed to raise the temperature of 1 g of a substance by 1 K, Hess's Law, the enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions and states of reactants and products are the same for each route, exact bond energy, the energy needed to break a specific covalent bond in a named molecule in the gaseous state, e.g. the O-H bond in water

Chapter 6 Definitions

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