Energetics I------------------------------------------------------------------------------------------------------
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Enthalpy
Heat energy change measured at a constant pressure. (H)
Endothermic
take in energy from surroundings
Exothermic
give out energy to their surroundings
ΔH
enthalpy change
Standard conditions (e)
‘standard’ at which enthalpy changes are measured and are: 100kPa, 298K
Calorimetry
an experimental method to find the enthalpy change in a chemical reaction
Standard enthalpy of combustion
enthalpy change when 1 mole of a substance burns completely in oxygen under standard conditions (298K, 100kPa) with all reactants and products in their standard states
Standard enthalpy of formation
enthalpy change when one mole of a substance forms from its constituent elements under standard conditions (298K, 100kPa) with all reactants and products in their standard states
Standard enthalpy of neutralisation
enthalpy change when one mole of water is produced in a neutralisation reaction between an acid and an alkali under standard conditions (298K, 100kPa) (NOT standard states)
Standard enthalpy of reaction
enthalpy change when the number of moles of substances shown by an equation as written react under standard conditions (298K, 100kPa) with all reactants and products in states GIVEN
Hess’ Law
states that the enthalpy change for a given reaction is the same, independent of the route by which this is achieved (provided the temperatures, pressures, and physical states of products and reactants are the same)
Bond enthalpy
the energy required to break one mole of bonds, in the gaseous state
Mean bond enthalpy
the energy required to break one mole of bonds, in the gaseous state, averages across a range of compounds