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Thermochemistry & Thermodynamics

13 terms

A–Z
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Endergonic Reaction Thermochemistry & Thermodynamics kJ/mol A reaction with a positive Gibbs free energy change, which requires an input of energy to proceed. ΔG > 0 Enthalpy Thermochemistry & Thermodynamics kJ/mol A thermodynamic state function equal to internal energy plus the product of pressure and volume. H = U + pV Enthalpy Level Diagram Thermochemistry & Thermodynamics kJ/mol A diagram plotting the enthalpies of reactants and products to show the direction and size of the enthalpy change. Enthalpy of Atomisation Thermochemistry & Thermodynamics kJ/mol The enthalpy change when one mole of gaseous atoms is produced from an element in its standard state. ΔH_at° Enthalpy of Dilution Thermochemistry & Thermodynamics kJ/mol The enthalpy change when a solution is diluted from one concentration to another by adding solvent. ΔH_dil Enthalpy of Fusion Thermochemistry & Thermodynamics kJ/mol The enthalpy change when one mole of a solid melts to a liquid at its melting point. ΔH_fus Enthalpy of Neutralisation Thermochemistry & Thermodynamics kJ/mol The enthalpy change when an acid and a base react to form one mole of water under standard conditions. H⁺ + OH⁻ → H₂O, ΔH = −57.1 kJ Enthalpy of Reaction Thermochemistry & Thermodynamics kJ/mol The heat absorbed or released when a reaction occurs at constant pressure in the molar amounts of the balanced equation. ΔH_rxn = ΣΔH_f(products) − ΣΔH_f(reactants) Enthalpy of Sublimation Thermochemistry & Thermodynamics kJ/mol The enthalpy change when one mole of a solid converts directly into vapour. ΔH_sub = ΔH_fus + ΔH_vap Enthalpy of Vaporisation Thermochemistry & Thermodynamics kJ/mol The enthalpy change when one mole of a liquid becomes vapour at its boiling point. ΔH_vap Entropy Thermochemistry & Thermodynamics J/(mol·K) A measure of the dispersal of energy and the number of microscopic arrangements available to a system. S = k ln W Entropy Change of the Surroundings Thermochemistry & Thermodynamics J/K The entropy change experienced by the surroundings when they absorb or release heat from a system. ΔS_surr = −ΔH_sys / T Exergonic Reaction Thermochemistry & Thermodynamics kJ/mol A reaction with a negative Gibbs free energy change, which therefore releases usable energy and proceeds spontaneously. ΔG < 0