Module 3 - Energy Flashcards
Exothermic
A reaction in which the enthalpy change of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings.
Enthalpy, H
The heat content that is stored in a chemical system.
Endothermic
A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, resulting in heat being taken in from the surroundings.
Enthalpy profile diagram
A diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products.
Activation energy
The minimum energy required to start a fraction by the breaking of bonds.
Standard conditions
S pressures of 100 kPa (1 atmosphere) and a stated temperature, usually 298K, and a concentration of 1.0 mol dm^-3 (for reactions with aqueous solutions).
Standard state
The physical state of a substance under standard conditions of 100kPa and 298K.
Standard enthalpy change of reaction
The enthalpy change that accompanies a few action in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states.
Standard enthalpy change of combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states.
Standard enthalpy change of formation
The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.
Unit for enthalpy changes
kJ mol^-1
Specific heat capacity, c
The nergy required to raise the temperature of 1g of a substance by 1 degree Celsius.
Bond enthalpy
The enthalpy change that takes place when breaking by homolytic fission 1 mole of a give bond in the molecules of a gaseous species.
Average bond enthalpy
The average enthalpy change that takes place when breaking by homolytic fission 1 mol of a given type of bond in the molecules of a gaseous species.
Hess’ law
‘If a reaction can take place by more than none route and the initial and final conditions are the same, the total enthalpy change is the same for each route.’