1. Calorimetry
Definition: Calorimetry is the accurate and precise measurement of heat flow for chemical and physical processes.
It operates under the law of conservation of energy (what is that?)
Heat loss = Heat gained
A device used to measure the absorption or release of this heat is called Calorimeter
Watch a video lecture for an example.

2. Types of Calorimeters:
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Constant-Pressure Calorimeter (simple calorimeter)
Because it is open to a constant atmospheric pressure
Heat content of a system at constant pressure is know as Enthalpy (H) of the system
Change in Enthalpy (ΔH) measures the amount of heat release or absorbed by a reaction at constant pressure.
q= ΔH

3. MEASURING ENTHALPY CHANGE
Minimizing Heat loss in a simple calorimeter
Convection
Radiation
Conduction
MEASURING ENTHALPY CHANGE
q= CmΔT
qsys = -qsurr
-qsys = qsurr
qsys = ΔH = -qsurr = - m. C. ΔT
ΔH = - m. C. ΔT
ΔH = negative = exothermic
ΔH = positive = endothermic
Discuss system and surroundings: Demo vinegar and Baking soda. Simulation Phet. Sources of energy

4. Types of Calorimeters:
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Constant-Volume Calorimeter (Bomb calorimeter)
Bomb calorimeter is an insulated device containing a sealed vessel used to measure the heat released during a combustion reaction.
It is the most reliable device for measuring specific heat of a substance
It is performed at constant volume of oxygen at high pressure.

5. Thermochemical equation
A chemical equation that includes the enthalpy change (ΔH)