Chemistry Exothermic and Endothermic Reactions

Exothermic Reactions

• Exothermic reactions release energy to the surroundings, increasing their temperature.
• Example: Wood burning, which is a form of combustion.
• Other examples include certain oxidation reactions and neutralization.
• Energy profile diagrams illustrate these energy changes, showing products with lower energy than reactants.
• The energy difference between reactants and products indicates the amount of energy released.
• Practical applications include hand warmers and self-heating food and drink containers.

Endothermic Reactions

• Endothermic reactions absorb energy from their surroundings, resulting in a decrease in temperature.
• Example: Thermal decomposition reactions.
• Energy profile diagrams for endothermic reactions show products with higher energy than reactants.
• The energy difference reflects the amount of energy absorbed by the reaction.

Activation Energy

• The activation energy is the minimum energy required for particles to collide and react.
• It appears as a peak in both exothermic and endothermic energy profiles.
• Activation energy can be graphically represented as the energy from the reactants to the peak of the energy curve.

Exothermic Reactions

• Energy is released to the surroundings, leading to a temperature increase.
• Wood burning serves as a classic example of combustion, which is an exothermic reaction.
• Other common examples are certain oxidation reactions and neutralization processes.
• Energy profile diagrams for exothermic reactions depict products that have lower energy than the reactants.
• The energy difference in these diagrams indicates the quantity of energy released during the reaction.
• Applications include hand warmers and self-heating food/drink containers that utilize the released energy.

Endothermic Reactions

• These reactions absorb energy, resulting in a temperature drop in their surroundings.
• A typical example is thermal decomposition, where a compound breaks down into simpler compounds.
• Energy profile diagrams for endothermic reactions exhibit products with higher energy compared to reactants.
• The difference in energy shows the amount of energy the system absorbs from the surroundings during the reaction.

Activation Energy

• Activation energy is the minimum energy threshold needed for particles to react upon collision.
• It is represented as a peak in energy profile diagrams, visible in both exothermic and endothermic reactions.
• Graphically, activation energy can be viewed as the energy required to move from the initial reactants' state up to the peak energy level.

Explore the fascinating world of chemical reactions with a focus on exothermic and endothermic processes. Learn key concepts such as energy release and absorption, practical applications, and activation energy. Test your knowledge on energy profile diagrams and real-life examples of these reactions.