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Chapter 1: Problem 13

Which of the following reasons correctly explains one reason that increasing the temperature of a reaction increases its speed? (A) All reactant molecules will have more kinetic energy. (B) A larger percentage of reactant molecules will exceed the activation energy barrier. (C) A higher percentage of molecular collisions will have the correct orientation to cause a reaction. (D) The order of each reactant will increase.

Short Answer

Expert verified
The correct answer is (B). A larger percentage of reactant molecules will exceed the activation energy barrier when temperature is increased. This is the predominant factor in increasing the speed of a reaction with a rise in temperature.

Step by step solution

01

Understanding the Impact of Temperature on Reactant Molecules Kinetic Energy

With an increase in temperature, the kinetic energy of the reactant molecules indeed increases. This causes the molecules to move around more swiftly. However, this is not the primary reason for the acceleration of the reaction.
02

Understanding the Effect of Temperature on Activation Energy

The activation energy is the minimum energy required for a reaction to occur. As temperature increases, a greater proportion of reactant molecules have sufficient energy to surpass this activation energy barrier. This is the primary reason an increase in temperature increases the speed of a reaction.
03

Understanding the Effect of Temperature on Molecular Collision Orientation

Temperature does not directly influence the orientation of the colliding molecules. Hence, it is not the primary cause of the increased reaction speed due to elevated temperature.
04

Understanding the Effect of Temperature on Reaction Order

Reaction order refers to the dependence of the reaction rate on the concentration of the reactants. It is an inherent characteristic of the reaction and is not directly influenced by changes in the temperature. Thus, it will not affect the speed of the reaction when temperature changes.

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