The energy needed to get a reaction started is referred to as: a. adhesion energy b. activation energy c. cohesion energy d. chemical energy
The Correct Answer and Explanation is:
The correct answer is b. activation energy.
Activation energy (Ea) is the energy required to initiate a chemical reaction. It is the minimum energy needed for reactants to collide and overcome the energy barrier that exists for the reaction to proceed. This energy is necessary to break bonds in the reactants, which is a prerequisite for the formation of new bonds in the products.
In chemical reactions, molecules must collide with sufficient energy and proper orientation for a reaction to occur. This is because atoms in molecules are held together by bonds, and breaking these bonds requires energy input. The activation energy represents the energy barrier that must be overcome for the reaction to proceed.
For example, when a match is struck, the friction generates heat, which provides the activation energy needed to ignite the chemicals in the match head. Similarly, in a laboratory setting, heating a mixture or using a catalyst can help overcome the activation energy barrier to allow the reaction to proceed.
Activation energy plays a significant role in determining the rate of a reaction. A high activation energy means the reaction will proceed slowly because fewer molecules have enough energy to overcome the barrier, whereas a lower activation energy means the reaction can occur more rapidly. Enzymes in biological systems often act as catalysts by lowering the activation energy, allowing reactions to occur more efficiently at body temperature.
To summarize, activation energy is crucial for determining how fast or slow a chemical reaction will occur and for understanding how reactants transform into products in various chemical processes.
