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Energetics - unit 5

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Harvey Buckle

on 10 August 2016

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Transcript of Energetics - unit 5

Lots of chemical reactions give out energy as heat. Getting heat by burning a fuel is a simple example, but you will probably have come across lots of others in the lab.

Other reactions need a continuous supply of heat to make them work. Splitting calcium carbonate into calcium oxide and carbon dioxide is a simple example of this.

Any chemical reaction will involve breaking some bonds and making new ones. Energy is needed to break bonds, and is given out when the new bonds are formed. It is very unlikely that these two processes will involve exactly the same amount of energy - and so some energy will either be absorbed or released during a reaction.
Heat 2
Heat is a form of _______. It is measured by the ____ k______ _____ of the particles in the SYSTEM.
A system is a reaction vessel or a place where a reaction is taking place.
Exothermic reaction
Endothermic reaction
A real example
Under discussion:
Heat is a form of energy. • Temperature is a measure of the average kinetic energy of the particles. • Total energy is conserved in chemical reactions. • Chemical reactions that involve transfer of heat between the system and the surroundings are described as endothermic or exothermic. • The enthalpy change (∆H) for chemical reactions is indicated in kJ mol-1
Make as many words as you can out of the word 'energetics'
Energetics - unit 5
Energy profiles
To know how reations can exchange energy
To demonstrate this with some reactions
8th August 2016
An experiment
Watch the board and complete energy profiles for all of the reactions and calculate the enthalpy changes
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