3.1.8 Thermodynamics

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18 Terms

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Hess’ Law

The enthalpy change for a chemical reaction is the same regardless of the route from reactants to products.

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Standard enthalpy of formation

The enthalpy change when one mole of a compound is formed from its elements under standard conditions and standard states.

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Standard enthalpy of combustion

The enthalpy change when one mole of a compound is burned completely in oxygen under standard conditions (EXOTHERMIC).

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Standard enthalpy of atomisation

The enthalpy change when one gaseous atom is formed from its element in standard state (ENDOTHERMIC).

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First ionisation enthalpy

The standard enthalpy change when one mole of electrons is removed from one mole of gaseous atoms to give the atom a positive charge (ENDOTHERMIC).

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Second ionisation enthalpy

The standard enthalpy change when one mole of electrons is removed from a +1 gaseous ion to form a gaseous ion with a 2+ charge (ENDOTHERMIC).

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First electron affinity

The standard enthalpy change when one mole of gaseous ions is converted to a gaseous ion with a -1 charge under standard conditions (EXOTHERMIC).

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Second electron affinity

The standard enthalpy change when one mole of electrons is added to a gaseous ion with a -1 charge to form an ion with a 2- charge.

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Lattice formation enthalpy

The standard enthalpy change when one mole of solid ionic compound is formed from its gaseous ions (EXOTHERMIC).

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Lattice dissociation enthalpy

The standard enthalpy change when one mole of solid ionic compound dissociates into gaseous ions (ENDOTHERMIC).

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Standard enthalpy of hydration

The standard enthalpy change when one mole of gaseous ions is converted into one mole of aqueous ions (EXOTHERMIC).

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Standard enthalpy of solution

The standard enthalpy change when one mole of solute dissolves in solvent to form a solution where the ions are too far to interact.

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Mean bond enthalpy

The enthalpy change when one mole of gaseous molecules breaks a covalent bond to form two free radicals (ENDOTHERMIC).

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Born-Haber cycle

A thermodynamic cycle that relates the enthalpy changes involved in the formation of an ionic compound from its elements.

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Perfect ionic model

A theoretical model where ions are considered as point charges and perfect spheres with no covalent character.

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Entropy

The amount of disorder within a system, always positive, and measured in JK⁻¹mol⁻¹.

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Gibbs free-energy change

A measure that determines whether a chemical reaction is feasible, calculated as ΔG = ΔH - TΔS.

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Feasibility of a reaction

A reaction is feasible if the Gibbs free-energy change is equal to or less than 0.