3.2 Flashcards
What happens in an exothermic reaction
- the enthalpy of the products is smaller than the enthalpy of the reactants
- heat loss from chemical system to surroundings
- △H has a - sign because heat has been lost by the chemical system
- Z shaped graph
What happens in a endothermic reaction
- the enthalpy of the products is greater than the enthalpy of the reactants
- there is a heat gain to the chemical system from the surroundings
- △H has a + sign because heat has been gained by the chemical system
- S shaped graph
Define activation energy
The minimum energy required to start a reaction by breaking bonds in the reactants
What are standard conditions
Standard set of conditions for experimental measurements established to allow comparisons to be made between different sets of data
100kPa
298K
What does it mean by standard states
All substances are in their standard states, i.e. their most stable form.
Define enthalpy change of reaction
The energy change associated with a given reaction
Define enthalpy change of formation
The energy change that takes place when 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 associated with the formation of 1 mole of water from a neutralisation reaction under standard conditions
q=mc△t stands for
q = heat exchanged w surroundings (J) m= mass of substance (WATER) heated or cooled c= specific heat capacity t= change in temperature measured in kelvin (K)
Explain average bond enthalpy
The mean energy needed for 1 mole of a given type of gaseous bonds to undergo homolytic fission
How do you predict enthalpy change
△H = Σ(bond enthalpies of reactants) - Σ(bond enthalpies of products)
Describe how a chemical reaction takes place in terms of bonds broken and made
- reactant bonds broken, takes in energy, endothermic
- atoms rearrange to form products
- product bonds formed, releases energy, exothermic change
What is Hess’ Law
Hess’ Law states that the enthalpy change in a chemical reaction is independent of the route it takes
What is an enthalpy cycle
An enthalpy cycle is a pictorial representation showing alternative routes between reactants and products