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Chapter 59: Problem 11

Provide two reasons (at least) why all collisions between molecules might not be effective in causing a reaction.

Short Answer

Expert verified
The two main reasons why all molecular collisions do not lead to a reaction are: lack of sufficient activation energy, and wrong orientation at the time of collision.

Step by step solution

01

Understanding the Minimum Energy Requirement

Molecules need to have at least a certain amount of energy, known as the activation energy, to cause a reaction when they collide. If the colliding molecules do not have this minimum level of energy, the reaction will not occur, even though a collision has taken place.
02

Considering the Orientation of Molecules

Even if the molecules have enough energy, they must collide in a particular orientation for a reaction to occur. This is because only certain parts of the molecules are involved in making and breaking bonds. If they collide in an orientation that doesn't allow these parts of the molecules to come into contact, the reaction will not occur.

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Most popular questions from this chapter

Which is more likely to weaken or break the bond between the nitrogen atom and the bromine atom in ONBr-a violent collision between two ONBr molecules or a gentle collision between two ONBr molecules? Explain.

Is a violent collision between two ONBr molecules more likely to occur at a high temperature or at a low temperature?

What is the mathematical relationship between \(E_{\mathrm{a}}\) (forward), \(E_{\mathrm{a}}\) (reverse), and \(\Delta H\) ?
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