How would the fraction of successful collisions change with an increase in reaction temperature?
A. The fraction of successful collisions would decrease.
B. The fraction of successful collisions would remain unchanged.
C. The fraction of successful collisions would increase.
D. The fraction of successful collisions would approach zero.
C. The fraction of successful collisions would increase.
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D. The fraction of successful collisions would approach zero.
But hey, look on the bright side! At least those unsuccessful collisions would be really good at becoming great icebreakers at parties. "Hey, remember that time we collided but nothing happened? Good times."
The correct answer is C. The fraction of successful collisions would increase.
When the reaction temperature increases, the kinetic energy of the particles involved in the reaction also increases. This increased kinetic energy leads to faster particle movement and more frequent collisions between the reactant molecules.
As the temperature increases, the average kinetic energy of the particles increases, which results in an increased frequency of collisions with sufficient energy to overcome the activation energy barrier for the reaction. These collisions are known as successful collisions because they lead to a chemical reaction.
Therefore, with an increase in reaction temperature, the fraction of successful collisions would increase because there would be a higher proportion of collisions with enough energy to result in a reaction.
To understand how the fraction of successful collisions changes with an increase in reaction temperature, we need to look at the concept of activation energy.
In a chemical reaction, particles must collide with sufficient energy (referred to as activation energy) and correct orientation to break the existing bonds and form new ones. Not all collisions have enough energy to overcome the activation energy barrier and result in a successful reaction. Therefore, the fraction of successful collisions affects the rate of the reaction.
Now, let's consider how increasing the reaction temperature affects the fraction of successful collisions:
1. As temperature increases, the average kinetic energy of the reacting particles also increases. This means that the particles move faster and collide more frequently.
2. With higher collision frequency, there is a greater probability of successful collisions occurring, as more collisions will have enough energy to overcome the activation energy barrier.
3. Additionally, when temperature increases, the distribution of kinetic energies among the particles shifts towards higher values. This implies that a larger fraction of colliding particles will possess the required energy to overcome the activation energy barrier.
Based on these points, we can conclude that the fraction of successful collisions would increase with an increase in reaction temperature. Therefore, the correct answer is C.