Question
The activation energy of a chemical reaction is +80 kJ and the enthalpy is +50 k. If the energy of collision of reactants is +60 kJ, will the reaction occur or not? Explain your answer written like an 8th grader
Answers
GPT-4o mini
To determine if a chemical reaction will occur, we need to consider two main energy factors: the **activation energy (Ea)** and the **energy of the collision** between the reactants.
1. **Activation Energy (Ea)**: This is the minimum amount of energy needed for the reactants to start the reaction. In this case, the activation energy is +80 kJ. This means that the reactants need at least 80 kJ of energy to make the reaction happen.
2. **Energy of Collision**: This is the energy that the reactants have when they collide with each other. In this scenario, the energy of collision is +60 kJ. This means that when the reactants bump into each other, they only have 60 kJ of energy.
Now, let’s compare the energy of the collision (60 kJ) to the activation energy (80 kJ):
- Since **60 kJ (collision energy)** is **less than 80 kJ (activation energy)**, the reactants do not have enough energy to overcome the energy barrier needed for the reaction to occur.
Therefore, since the energy of the collision is not high enough to meet the activation energy requirement, **the reaction will NOT occur**.
1. **Activation Energy (Ea)**: This is the minimum amount of energy needed for the reactants to start the reaction. In this case, the activation energy is +80 kJ. This means that the reactants need at least 80 kJ of energy to make the reaction happen.
2. **Energy of Collision**: This is the energy that the reactants have when they collide with each other. In this scenario, the energy of collision is +60 kJ. This means that when the reactants bump into each other, they only have 60 kJ of energy.
Now, let’s compare the energy of the collision (60 kJ) to the activation energy (80 kJ):
- Since **60 kJ (collision energy)** is **less than 80 kJ (activation energy)**, the reactants do not have enough energy to overcome the energy barrier needed for the reaction to occur.
Therefore, since the energy of the collision is not high enough to meet the activation energy requirement, **the reaction will NOT occur**.