100 kPa or 1 atm. pressure and a temperature of 298 K or 25°C
Why are standard conditions required?
To enable comparison
In and exothermic reaction is enthalpy change a positive or negative value?
negative
In an exothermic reaction:
• The chemical system loses energy
• The surroundings gains energy
• The temperature of the surroundings increase
In an endothermic reaction:
• The chemical system gains energy
• The surroundings loses energy
• The temperature of the surroundings decrease.
Definition of activation energy.
is the minimum energy needed to start a reaction by the breaking of bonds
How is activation often provided?
heating or a spark
Definition of standard enthalpy of formation.
Enthalpy change of formation (ΔfH) - The enthalpy change that takes place when one mole of a compound in its standard state is formed from its constituent elements in their standard states under standard conditions.
Definition of standard enthalpy of combustion.
Enthalpy change of combustion (ΔcH) - The enthalpy change when one mole of an element or compound reacts completely with oxygen under standard conditions.
Definition of standard enthalpy change of reaction.
Standard Enthalpy Change of Reaction (ΔrH) - The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions.
Definition of the enthalpy change of neutralisation.
Enthalpy change of neutralisation (ΔnH) - The change in enthalpy that occurs when one equivalent of an acid and one equivalent of a base undergo a neutralisation reaction to form water and a salt. It is defined as the energy released with the formation of 1 mole of water.
What apparatus is used to measure ethalpy change?
calorimeter
What 3 measurements are taken when carrying out an experiment for enthalpy change.
Initial and final temperature to workout the change
Volume of solution or amount of water where the temperature change occurs
number of moles of reactants
What is the equation for energy change?
Energy change = m c ∆T
What is the equation for the enthalpy change per mole.
energy change/moles of substance used
Simple experiments to measure enthalpy of combustion often produce results that are less than the accepted (literature) values.
Suggest 3 reasons why this may be the case.
• heat loss to environment
• Incomplete combustion of fuel
• Evaporation of fuel from wick
• Non standard conditions
List 3 reasons that make the bomb calorimeter an improvement over the calorimeter we would use in our laboratory.
• No heat loss
• No evaporation of fuel
• Plenty of O2 supplied so incomplete combustion less likely.