Energy in Chemical ReactionsChemical reactions involve energy changes. Some release energy, while others absorb energy.
visually show how energy changes during a reaction. They indicate:
- Exothermic Reactions: These reactions release heat energy into the surroundings, causing a temperature increase. Examples include combustion, respiration, and neutralization reactions.
- Endothermic Reactions: These reactions absorb heat energy from the surroundings, causing a temperature drop. Examples include photosynthesis and thermal decomposition.
- Activation Energy: This is the minimum amount of energy needed to start a reaction. It is required to break bonds in the reactants before new bonds can form in the products.
visually show how energy changes during a reaction. They indicate:
- The energy of reactants and products
- The activation energy peak
- Whether the reaction is exothermic (energy decreases) or endothermic (energy increases)
Energy in Chemical Reactions (Simplified)Chemical reactions involve energy. Some reactions give out energy, and others take in energy.
- Exothermic Reactions: These give out heat and make things warmer. Example: burning wood or fireworks exploding.
- Endothermic Reactions: These take in heat and make things cooler. Example: melting ice or cooking food.
- Activation Energy: This is the energy needed to start a reaction—like a match needed to light a candle.
