module 3: 9.1 enthalpy changes Flashcards
3.2.1 enthalpy changes
define the term enthalpy
enthalpy (H) is a measure of the heat content or energy in a chemical system. The chemical system refers to the atoms, molecules or ions making up the chemicals.
what is an exothermic change
- from the system to the surroundings, it releases heat energy to the surroundings.
- Delta H is negative
- The temperature of the surroundings increase as they gain energy (temp increase)
- Reactants is higher than products
what is an endothermic change
- from the surroundings to the system, it takes in heat energy from the surroundings
- Delta H is positive
- The temperature of the surroundings decrease as they lost energy (temp decrease)
- Reactants is lower than products
define the term activation energy
the energy required to break bonds acts as an energy to the reaction, known as activation energy E (subscript) a
It is the minimum energy needed for the reaction to take place
what are the standard conditions
- standard pressure - 100 kPa
- standard temperature - 25 degrees C or 298 K
- standard concentration - 1 mol dm-3
standard state - physical state under standard conditions
define the standard enthalpy change of reaction
the standard enthalpy change of reaction (ΔrH^⦵) is the enthalpy change that accompanies a reaction in the molar quantities shown in a chemical equation under standard conditions, with all reactants and produces in their standard states
define the enthalpy change of formation
the standard enthalpy change of formation (ΔfH^⦵) is the enthalpy change that takes place when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states
define enthalpy change of combustion
the standard enthalpy change of combustion (ΔcH^⦵) is the enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states.
define enthalpy change of neutralisation
the standard enthalpy change of neutralisation (ΔneutH^⦵) is the energy change that accompanies the reaction of an acid by a base to form one mole of H20 (l), under standard conditions, with all reactants and products in their standard states.
formula for energy (Q)
Q = mcΔT q - energy (J) m - mass of water c - 4.18 (J/g/ degrees C or K) ΔT - Change in temperature (degrees C)