Enthalpy Changes Flashcards
What does system mean in a chemical reaction?
The atoms and bonds involved in the chemical reaction.
Explain the law of conservation.
The amount of energy in an isolated system remains the same. Energy cannot be created or destroyed, it can only be transferred from one form to another.
What energy change is breaking bonds associated with?
Energy is taken in to break bonds —> endothermic reaction
What energy change is making bonds associated with?
Energy is released to make bonds —> exothermic reaction
What is an endothermic reaction?
A reaction with an overall positive enthalpy change (+ΔH) —> enthalpy of products > enthalpy of reactants
What is an exothermic reaction?
A reaction with an overall negative enthalpy change (-ΔH) —> enthalpy of products < enthalpy of reactants
What does activation energy mean?
The minimum energy required for a reaction to take place
What are the standard conditions?
100 kPa
298 K
What does ‘in standard state’ mean?
The state and element / compound exists at in standard conditions
Define enthalpy change of formation.
The energy change that takes 1 mole of a compound is formed from its constituent elements in their standard state under standard conditions
Define enthalpy change of combustion
The energy change that takes place when 1 mole of a substance is completely combusted.
Define enthalpy change of neutralisation
The energy change that takes place when 1 mole of water is formed from a neutralisation reaction.
What does the enthalpy change of reaction mean?
The energy change associated with a given reaction.
What are the advantages of using a bomb calorimeter? (2)
- minimises heat loss
- pure oxygen used —> ensures complete combustion
Why might experimental methods for enthalpy determination not be accurate?
Heat is lost to surroundings
Not in standard conditions
Reaction mau not go to completion