Which of the following statements is true if HI is formed in the following reaction?
H2(g) + I2(g) → 2HI(g)
a. There are no collisions between the reactants in the reaction
b. All of the collisions between reactants have enough energy to overcome the activation energy.
c. Some of the collisions between reactants have enough energy to overcome the reaction mechanism.
d. Some of the collisions of the reactants have enough energy to overcome the activation energy.
To determine which of the statements is true if HI is formed in the given reaction, we need to understand the concept of collision theory.
Collision theory states that for a reaction to occur, the reactant particles must collide with each other. Additionally, these collisions must have sufficient energy to overcome the activation energy barrier, allowing the reactant molecules to react and form the product.
In the given reaction, H2(g) + I2(g) → 2HI(g), the reactant molecules H2 and I2 collide with each other to form the product HI. Since HI is formed, that means the reaction has occurred.
Now, let's evaluate each statement:
a. There are no collisions between the reactants in the reaction.
This statement is false because, according to collision theory, reactions require collisions between reactant particles for the reaction to occur. Since HI is formed, there must have been collisions between H2 and I2.
b. All of the collisions between reactants have enough energy to overcome the activation energy.
This statement is false. According to collision theory, not all collisions have enough energy to overcome the activation energy barrier. Only collisions with sufficient energy, equal to or greater than the activation energy, can proceed to form products. This is why not all particles involved in a reaction will react upon collision.
c. Some of the collisions between reactants have enough energy to overcome the reaction mechanism.
This statement does not accurately describe the situation. The term "reaction mechanism" refers to the detailed series of steps involved in a chemical reaction, which usually involves intermediate species. The statement does not consider the activation energy barrier specifically.
d. Some of the collisions of the reactants have enough energy to overcome the activation energy.
This is the correct statement. According to collision theory, only collisions that possess sufficient energy to overcome the activation energy barrier result in the formation of HI. Therefore, some of the collisions between the reactant molecules (H2 and I2) must have had enough energy to overcome the activation energy.
In conclusion, the correct statement is:
d. Some of the collisions of the reactants have enough energy to overcome the activation energy.