The balance between the Energy needed to break bonds and the Energy released when new bonds are made is what decides whether a reaction is endothermic or exothermic. We can find out more about what is happening in a particular reaction by looking at Energy level diagrams.
Energy level diagrams show us the relative amounts of Energy contained in the reactants and the products of this reaction. This Energy is measured in kJ/mol.
The difference between the Energy levels of the reactants and the products is the change during the reaction, measured in kJ/mol. We represent this Energy change by the symbol ΔH ('Delta H'). This simply means 'the difference in Energy between the products and the reactants'.
- In an exothermic reaction, the 'ΔH' is always negative, because the products are at a lower Energy level than the reactants. The temperature of the surroundings increases.
- In an endothermic reaction, the 'rg' is always positive, because the products are at a higher Energy level than the reactants. The temperature of the surroundings decreases.
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