The loss of heat energy by a system; enthalpy change is negative
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Endothermic
the gain of heat energy by a system; the enthalpy change is possitive v
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Enthalpy change
the amount of heat energy released or absorbed when a chemical or physical change occurs at constant pressure + sign
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standard enthalpy of combustion
the enthalpy change, under standard conditions, when 1 mol of a substance is burned completely in oxygen, with all reactants and products in their standard states
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standard enthalpy of formation
the enthalpy change, under standard conditions, when 1 mol of a compound is formed from its elements, with all reactants and products in their standard states
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standard states
the normal, stable state of an element or compound under standard conditions, usually 298 K and 100 kPa
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specific heat capacity, c
the amount of heat needed to raise the temperature of 1g of substance by 1K. Its units are joules per gram per kelvin
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calorimeter
apparatus used to measure heat change
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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
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enthalpy of elements
The enthalpies of all elements in their standard states are taken as zero
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allotropes
different structural modifications of an element
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Bond dissociation enthalpy
the enthalpy change for the breaking of a covalent bond with all species in the gaseous state
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mean bond enthalpy
the average of several values of the bond dissociation enthalpy for a given type of bond, taken from a range of different compounds
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Other cards in this set
Card 2
Front
the gain of heat energy by a system; the enthalpy change is possitive v
Back
Endothermic
Card 3
Front
the amount of heat energy released or absorbed when a chemical or physical change occurs at constant pressure + sign
Back
Card 4
Front
the enthalpy change, under standard conditions, when 1 mol of a substance is burned completely in oxygen, with all reactants and products in their standard states
Back
Card 5
Front
the enthalpy change, under standard conditions, when 1 mol of a compound is formed from its elements, with all reactants and products in their standard states
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