As time goes on, a reaction may slow down due to several factors related to the collision theory. The collision theory states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Here are the steps to explain why a reaction slows down over time using ideas from the collision theory:

1. Decrease in reactant concentration: As the reaction progresses, the concentration of reactant particles decreases. With fewer particles available, the chances of successful collisions between reactant particles also decrease. This leads to a slower reaction rate.

2. Decrease in collision frequency: Over time, the number of collisions between reactant particles decreases. This can be attributed to the decrease in reactant concentration and the consumption of reactants as the reaction proceeds. With fewer collisions occurring, the reaction rate slows down.

3. Decrease in effective collisions: Not all collisions between reactant particles result in a successful reaction. Only collisions with sufficient energy and proper orientation lead to a reaction. As time goes on, the proportion of effective collisions decreases, leading to a slower reaction rate.

4. Increase in activation energy barrier: The collision theory also suggests that particles must possess a minimum amount of energy, known as activation energy, to overcome the energy barrier and initiate a reaction. As the reaction progresses, the concentration of reactants decreases, and the remaining reactant particles may have lower average energy. This increase in the activation energy barrier makes it more difficult for collisions to result in a successful reaction, causing the reaction rate to slow down.

Overall, the decrease in reactant concentration, collision frequency, and effective collisions, along with the increase in activation energy barrier, contribute to the slowing down of a reaction over time, as suggested by the collision theory.

Question

As time goes on, a reaction may slow down due to several factors related to the collision theory. The collision theory states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Here are the steps to explain why a reaction slows down over time using ideas from the collision theory:

1. Decrease in reactant concentration: As the reaction progresses, the concentration of reactant particles decreases. With fewer particles available, the chances of successful collisions between reactant particles also decrease. This leads to a slower reaction rate.

2. Decrease in collision frequency: Over time, the number of collisions between reactant particles decreases. This can be attributed to the decrease in reactant concentration and the consumption of reactants as the reaction proceeds. With fewer collisions occurring, the reaction rate slows down.

3. Decrease in effective collisions: Not all collisions between reactant particles result in a successful reaction. Only collisions with sufficient energy and proper orientation lead to a reaction. As time goes on, the proportion of effective collisions decreases, leading to a slower reaction rate.

4. Increase in activation energy barrier: The collision theory also suggests that particles must possess a minimum amount of energy, known as activation energy, to overcome the energy barrier and initiate a reaction. As the reaction progresses, the concentration of reactants decreases, and the remaining reactant particles may have lower average energy. This increase in the activation energy barrier makes it more difficult for collisions to result in a successful reaction, causing the reaction rate to slow down.

Overall, the decrease in reactant concentration, collision frequency, and effective collisions, along with the increase in activation energy barrier, contribute to the slowing down of a reaction over time, as suggested by the collision theory.

Knowee AI · Accepted Answer

As time goes on, a reaction may slow down due to several factors related to the collision theory. The collision theory states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Here are the steps to explain why a reaction slows down over time using ideas from the collision theory:

1. Decrease in reactant concentration: As the reaction progresses, the concentration of reactant particles decreases. With fewer particles available, the chances of successful collisions between reactant particles also decrease. This leads to a slower reaction rate.

2. Decrease in collision frequency: Over time, the number of collisions between reactant particles decreases. This can be attributed to the decrease in reactant concentration and the consumption of reactants as the reaction proceeds. With fewer collisions occurring, the reaction rate slows down.

3. Decrease in effective collisions: Not all collisions between reactant particles result in a successful reaction. Only collisions with sufficient energy and proper orientation lead to a reaction. As time goes on, the proportion of effective collisions decreases, leading to a slower reaction rate.

4. Increase in activation energy barrier: The collision theory also suggests that particles must possess a minimum amount of energy, known as activation energy, to overcome the energy barrier and initiate a reaction. As the reaction progresses, the concentration of reactants decreases, and the remaining reactant particles may have lower average energy. This increase in the activation energy barrier makes it more difficult for collisions to result in a successful reaction, causing the reaction rate to slow down.

Overall, the decrease in reactant concentration, collision frequency, and effective collisions, along with the increase in activation energy barrier, contribute to the slowing down of a reaction over time, as suggested by the collision theory.

Use ideas from the collision theory to suggest why a reaction slows down as time goes on.

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Use ideas from the collision theory to suggest why a reaction slows down as time goes on.

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