2.3 Flashcards
Exothermic
Reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings
Enthalpy
The heat content that is stored in a chemical system
Endothermic
Refers to 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
Activation energy
The minimum energy required to start a reaction by the breaking of bonds.
Standard conditions
A pressure of 100KPa a stated temperature usually 298K and a concentration of 1 moldm-3 ( for reactions with aqueous solutions
Standard state
The physical state of a substance under the standard conditions of 100KPa and 298K
Specific heat capacity
The energy required to raise the temperature of 1g of a substance by 1°c
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 reactant 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 it’s constituent elements
In their standard states all reactants and products being in their standard states.
Bond enthalpy
The enthalpy change that takes place when breaking by homolytic fission 1 mol of a given 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 one route and the initial and final conditions are the same, the total enthalpy change is the same for each route.
Rate of reaction
The change in concentration of a reactant or a product in a given time.
Standard enthalpy change of reaction
The enthalpy change that accompanies a reaction
In the molar quantities
Expressed in a chemical equation
Under standard conditions and all reactants and products being in their standard states.
Heterogenous catalysis
Catalysis of a reaction in which the catalyst has a different physical state from the reactants