True or false

1. The energy of a collision between atoms or molecules must be greater than the activation energy for bonds to be broken?

2. Decreasing the temperature decreases the kinetic energy of the reactant, and the reaction goes more slowly?

3. two or more atoms must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur?

4. If the heat of reaction is positive the energy of the product is lowere than the energy of the products is lower than the energy of the reactant and the reaction is exothermic?

5. Increasing the amount of reactants increases the number of collisions, and the reaction goes faster?

and what do you think and why? Surely you don't want us to give you the answers.

1. True

2. true
3. true
4. false
5. true

1. True. In order for chemical bonds to break and a reaction to occur, the energy of a collision between atoms or molecules must be greater than the activation energy. The activation energy is the minimum energy required for a reaction to proceed.

To understand this concept, you can refer to the Arrhenius equation. It states that the rate constant of a reaction is proportional to the exponential of the negative ratio of the activation energy to the product of the gas constant (R) and temperature (T). In other words, if the collision energy is below the activation energy, the reaction will not occur.

2. True. Decreasing the temperature will indeed reduce the kinetic energy of the reactant particles, resulting in slower reaction rates. This is due to the fact that temperature is directly related to the average kinetic energy of molecules. When the temperature decreases, the molecules move more slowly and collide less frequently, thus slowing down the overall reaction.

To visualize this effect, you can think of molecules as tiny particles in constant motion. Higher temperatures provide more energy to the molecules, making them move faster and increase the chances of successful collisions. Lower temperatures reduce this movement and, consequently, the reaction rate.

3. True. For a chemical reaction to occur, two or more atoms (or molecules) must collide with proper orientation and with energy greater than or equal to the activation energy. This concept is known as the collision theory.

When atoms or molecules collide, they need to have appropriate relative orientations for their bonds to break and reform in new configurations. Additionally, the collision energy must be sufficient to overcome the energy barrier represented by the activation energy. Only collisions that satisfy these conditions result in the occurrence of a reaction.

4. False. If the heat of reaction is positive, it means that the energy of the products is higher than the energy of the reactants. In such cases, the reaction is endothermic, not exothermic. Endothermic reactions absorb energy from their surroundings, leading to a decrease in temperature in the environment.

Exothermic reactions, on the other hand, have a negative heat of reaction. This indicates that the energy of the products is lower than the energy of the reactants. Exothermic reactions release energy, often in the form of heat, light, or sound, making the reaction surroundings warmer.

5. True. Increasing the amount of reactants generally increases the number of collisions between particles. As a result, the reaction rate tends to be faster. When there are more reactant particles available, there is a higher probability of successful collisions between them.

This observation can be explained using the collision theory. By increasing the amount of reactants, the chances of molecules colliding with sufficient energy and appropriate orientation for a reaction to occur are heightened. As a result, the frequency of successful collisions and the reaction rate increase.