DF Flashcards
exothermic reaction
reaction that gives out energy to the surroundings. delta H is - ve.
Energy released in making new bonds is greater than energy required to break existing bonds.
endothermic reaction
reaction that takes in energy from and cools the surroundings. delta H is + ve.
Energy released in making new bonds is less than energy required to break existing bonds.
standard conditions
298 K
1 atm pressure
1 mol dm-3 solutions
standard enthalpy change of reaction
enthalpy change when molar quantities of reactants as stated in the equation react together under standard conditions.
standard enthalpy change of combustion
enthalpy change when 1 mole of a substance is burnt completely in oxygen under standard conditions with elements in their standard states.
standard enthalpy change of formation
enthalpy change when 1 mole of a compound is formed from its elements under standard conditions in standard states.
standard enthalpy change of neutralisation
enthalpy change when 1 mole of H+ ions reacts with 1 mole of OH- ions to form 1 mole of water under standard conditions with 1 mol dm-3 solutions.
converting from celcius to kelvin and kelvin to celcius:
+ 273
- 273
aromatic compounds
compounds which contain 1 or more benzene rings
aliphatic compounds
compounds which do not contain any benzene rings
hydrocarbon
a compound formed of carbon and hydrogen atoms only
functional group
a modifier responsible for the characteristic chemical reactions of molecules.
saturated compound
hydrocarbons containing the maximum number of hydrogen atoms possible/ no C to C double or triple bonds.
homologous series
a series of compounds which all have the same general molecular formula and functional group.
average bond enthalpy
average quantity of energy required to break 1 mole of a bond with substances in the gaseous state. kJ mol-1