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Thermodynamics
AQA A Level Chemistry
Question | Answer |
---|---|
What does a negative free energy change tell us? | The process is spontaneous (feasible). |
Define enthalpy change | The heat change at constant pressure |
Define enthalpy of atomisation of an element. | The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state |
Define enthalpy of hydration. | The standard enthalpy change when water molecules surround one mole of gaseous ions. |
Define enthalpy of solution. | The standard enthalpy change when one mole of an ionic solid dissolves completely in sufficient water to form a solution in which the ions are far enough apart not to interact with each other |
Define first electron affinity. | The standard enthalpy change when a mole of gaseous atoms is converted to a mole of gaseous ions each with a single negative charge. |
Define first ionisation energy. | The standard enthalpy change when one mole of gaseous atoms is converted into a mole of gaseous ions each with a single positive charge. |
Define lattice dissociation enthalpy. | The standard enthalpy change when one mole of solid ionic compound is broken up into its free gaseous ions. |
Define lattice formation enthalpy. | The standard enthalpy change when one mole of solid ionic compound is formed from its free gaseous ions. |
Define mean bond enthalpy. | The enthalpy change when one mole of covalent bonds is broken, with all species in the gaseous state, average over a range of different compounds. |
Define second electron affinity. | The standard enthalpy change when a mole of electrons is added to a mole of gaseous ions each with a single negative charge to form ions each with a double negative charge. |
Define second ionisation energy. | The standard enthalpy change when one mole of gaseous unipositive ions is converted into a mole of gaseous ions each with a double positive charge. |
Define standard enthalpy of atomisation of a compound. | The enthalpy change when one mole of a compound in its standard state is converted into its free gaseous atoms. |
Define standard enthalpy of combustion. | The enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions, all reactants and products being in their standard states. |
Define standard enthalpy of formation. | The enthalpy change when one mole of a substance is produced from its constituent elements under standard conditions, all reactants and products being in their standard states. |
Define the Perfect Ionic Model. | A mathematical calculation of the lattice formation enthalpy of a compound, which assumes that the positive and negative ions are perfectly spherical and that there is no covalent character in the compound. |
State Hess's Law | The enthalpy change of a reaction depends only on the initial and final states of the reaction and is independent of the route by which the reaction occurs. |
What are standard conditions? | A standard pressure of 100 kPa and a stated temperature |
What is entropy? | A measure of disorder |
What is the entropy change? | The change in disorder of a system. An increase in disorder produces a positive entropy change. |