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14 Cards in this Set
- Front
- Back
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Enthalpy
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The heat content that is stored in a chemical system.
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Exothermic
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A reaction where the enthalpy of the products is smaller than the enthalpy of the reactants. Results in heat loss to surroundings.
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Endothermic
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A reaction where the enthalpy of the products is greater than the enthalpy of the reactants. Results in taking in heat from surroundings.
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Enthalpy Profile Diagram
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Diagram for a reaction to compare enthalpy of reactants with the enthalpy of the products.
(Includes Ea and enthalpy difference) |
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Activation Energy
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The minimum energy required to start a reaction by the breaking of bonds.
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Standard Conditions
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1 atmosphere, stated temperature (usually 298K) and 1.0 mol dm^-3.
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Standard State
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Physical state of a substance under standard conditions.
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Standard Enthalpy Change of Reaction
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The enthalpy change that accompanies a reaction in molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states.
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Standard Enthalpy Change of Combustion
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The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states.
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Standard Enthalpy Change of Formation
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The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.
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Specific Heat Capacity
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The energy required to raise the temperature of 1g of a substance by 1 degree celcius.
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Bond Enthalpy
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The enthalpy change that takes place when one mole of a specific bond in the molecules of a gaseous species.
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Average Bond Enthalpy
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The average enthalpy change that takes place when breaking 1 mole of a specific bond in the molecules of a gaseous species.
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Hess' Law
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If a reaction can take place by more than one route and the initial and final conditions are the same, then the total enthalpy change is the same for each route.
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