Open Question
What happens to the reaction rate as the reactants get used up in a reaction?
15. Chemical Kinetics
Factors Influencing Rates
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Which of the following best explains how increasing the concentration of reactants affects the reaction rate?
A
It changes the reaction mechanism to a faster pathway.
B
It decreases the activation energy required for the reaction.
C
It increases the temperature of the reaction mixture.
D
It increases the frequency of collisions between reactant molecules.
Verified step by step guidance1
Understand the concept of reaction rate: Reaction rate refers to how quickly a reaction occurs. It is influenced by several factors, including the concentration of reactants.
Consider the collision theory: According to collision theory, chemical reactions occur when reactant molecules collide with sufficient energy and proper orientation.
Analyze the effect of concentration on collisions: Increasing the concentration of reactants means there are more molecules present in a given volume, which leads to an increased likelihood of collisions between reactant molecules.
Relate concentration to reaction rate: With more frequent collisions, the chances of successful interactions that lead to product formation increase, thereby increasing the reaction rate.
Clarify why other options are incorrect: Changing the reaction mechanism, decreasing activation energy, or increasing temperature are not direct effects of increasing reactant concentration. The primary effect is the increased frequency of collisions.
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