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.
The answer is D
Well, that reaction looks like a wild party! So, let's see. If HI is formed in the reaction, it means that the reaction actually occurred. And if a reaction occurs, it means that some of the collisions of the reactants had enough energy to overcome the activation energy. So, I'd go with option d, because those reactants are definitely having a great time bumping into each other!
To determine which of the statements is true if HI is formed in the given reaction, let's discuss the concept of collision theory and activation energy.
In the context of chemical reactions, the collision theory explains that for a reaction to occur, reactant particles must collide with each other. However, not all collisions result in a successful reaction. Successful reactions depend on two factors: the collision frequency and the collision energy.
The collision frequency refers to the number of collisions happening per unit time. The more frequent the collisions, the higher the likelihood of a reaction occurring.
On the other hand, collision energy refers to the energy possessed by the colliding particles. For a reaction to occur, the colliding particles must possess enough energy, known as activation energy, to break the existing bonds and form new ones.
Now, let's analyze each statement:
a. There are no collisions between the reactants in the reaction.
This statement is false. In any chemical reaction, the reactant particles must collide for a reaction to occur. Hence, there must be collisions between the H2 and I2 molecules in this case.
b. All of the collisions between reactants have enough energy to overcome the activation energy.
This statement is unlikely to be true. In most chemical reactions, not all collisions possess sufficient energy to overcome the activation energy barrier. Only a fraction of the collisions have the required energy for a reaction to occur.
c. Some of the collisions between reactants have enough energy to overcome the reaction mechanism.
This statement is incorrect as it combines the concepts of activation energy and reaction mechanism. The reaction mechanism refers to the sequence of individual steps involved in a reaction, while activation energy pertains to the energy required for the reaction to proceed. Therefore, it is inappropriate to connect these two in this statement.
d. Some of the collisions of the reactants have enough energy to overcome the activation energy.
This statement is true. According to collision theory, only a fraction of all collisions possess sufficient energy to overcome the activation energy barrier. These collisions, referred to as effective collisions, lead to the formation of product molecules (in this case, HI).
In conclusion, the correct statement is d. Some of the collisions of the reactants have enough energy to overcome the activation energy.
The answer is C, some of the collisions between reactants have enough energy to overcome reaction mechanism.
I thought it was B since the reaction was 2 moles of each create 2 moles of the product but apparently not