Thermodynamics Definitions 0.0 / 5 ? ChemistryThermodynamicsInternational BaccalaureateOther Created by: Lotto65Created on: 06-03-17 19:31 Heat... A form of energy that flows from something at a higher temperature to something at a lower temperature 1 of 27 Temperature... A measure of the average kinetic energy of particles 2 of 27 Internal energy... The total amount of energy (kinetic and potential) in a sample of a substance 3 of 27 Exothermic reaction... A reaction where heat energy is transferred from a system to its surroundings 4 of 27 Endothermic reaction... A reaction where a system takes in heat energy from the surroundings 5 of 27 Enthalpy change... The amount of heat energy taken in or given out in a reaction 6 of 27 Enthalpy... The total energy stored in a substance 7 of 27 Stability... The relative energies of reactants and products in a chemical reaction 8 of 27 Standard enthalpy change of reaction... The enthalpy change when molar amounts of reactants react together under standard conditions 9 of 27 Standard enthalpy change of combustion... The enthalpy change when one mole of a substance is completely burnt in oxygen under standard conditions 10 of 27 Specific heat capacity... The energy required to raise the temperature of 1kg of a substance by 1K 11 of 27 Enthalpy change of neutralisation... The enthalpy change when one mole of water molecules are formed when an acid reacts with an alkali under standard conditions 12 of 27 Enthalpy change of solution... The enthalpy change when one mole of a solute is dissolved in excess solvent to form a solution of 'infinite' dilution under standard conditions 13 of 27 Infinite dilution... Any further dilution of the solution produces no further enthalpy change 14 of 27 Hess' law... The enthalpy change accompanying a chemical reaction is independent of the pathway between the initial and final states 15 of 27 Standard enthalpy change of formation... The enthalpy change when one mole of a substance is formed from its elements in their standard states under standard conditions 16 of 27 Standard state... A pure substance at 100kPa and a specified room temperature 17 of 27 Bond enthalpy... The enthalpy change when one mole of covalent bonds in a gaseous molecule are broken under standard conditions 18 of 27 Standard enthalpy change of vaporisation... The enthalpy change for a reaction involving the formation of one mole of gaseous molecules 19 of 27 Average bond enthalpy... The average amount of energy required to break one mole of covalent bonds, in gaseous molecules under standard conditions 20 of 27 Standard enthalpy change of atomisation... The enthalpy change when one mole of gaseous atoms is formed from an element under standard conditions 21 of 27 First ionisation energy... The enthalpy change when one electron is removed from each atom in one mole of gaseous atoms under standard conditions 22 of 27 First electron affinity... The enthalpy change when one electron is added to each atom in one mole of gaseous atoms under standard conditions 23 of 27 Lattice enthalpy... The enthalpy change when one mole of an ionic compound is broken apart into its constituent gaseous ions under standard conditions 24 of 27 Enthalpy change of hydration... The enthalpy change when one mole of gaseous ions is surrounded by water molecules to form an 'infinitely dilute solution' under standard conditions 25 of 27 Entropy... A measure of how the available energy is distributed among particles 26 of 27 Spontaneous reaction... One that occurs without any outside influence 27 of 27
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