Enthalpy change
Enthalpy change
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Types of reactions
Exothermic
Exothermic
Reaction that releases energy to the surroundings thus the products contains less energy than the reactants.
Endothermic
Endothermic
Reaction that absorbs energy from the surroundings thus the products contains more energy more than the reactants
Types of standard enthalpy changes
standard conditions: 10^5 Pa, 298K, The reactants and products must be in their standard states
Reaction
Reaction
The standard enthalpy change of reaction is the enthalpy change when the amounts of reactants shown in the equation react to give products under standard conditions.
Formation
Formation
The standard enthalpy change of formation is the enthalpy change when one mole of a compound is formed from its elements under standard conditions.
Combustion
Combustion
The standard enthalpy change of combustion is the enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions
Neutralization
Neutralization
The standard enthalpy change of Neutralization is the enthalpy change when one mole of water is formed by the reaction of an acid and alkali under standard conditions
Solution
Solution
The standard enthalpy change of solution is the enthalpy change when one mole of solute dissolves in a solvent to form an infinitely dilute solution under standard conditions
Atomization
Atomization
The standard enthalpy change of atomization is the enthalpy change when one mole of gaseous atoms is formed from its elements under standard conditions
anhydrous salt
anhydrous salt
The standard enthalpy change of anhydrous salt is the enthalpy change when one mole of hydrated salt is formed from one mole of the anhydrous salt under standard conditions
Hess's law and cycle
Hess's law and cycle
Hess's law states that the total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same
Hess's law states that the total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same
Bond enthalpy
Bond enthalpy
the amount of energy required to break one mole of the stated bond.
the amount of energy required to break one mole of the stated bond.
Recap:
Endothermic and Exothermic reactions
Endothermic and Exothermic reactions
part 2
part 2
standard enthalpy changes
standard enthalpy changes
Hess's law calculation
Hess's law calculation
Bond enthalpy
Bond enthalpy
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