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๐Ÿงชย ap chem

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๐Ÿ‘Ÿย Unit 5

ย ย โ€ขย ย โฑ๏ธ2 min read

5.6 Reaction Energy and Graphs w/ Energy

Dylan Black

dylan black

โฑ๏ธ June 2, 2020

๐Ÿ“…โŒจ๏ธ

๐ŸŽฅ Watch: Activation Energy

Energy In Reactions

Graphs of Energy w/ Respect to Reaction Progress

As you have probably seen, potential energy in a reaction can be represented as a curve with a hump as the reaction progresses, with energy changes being able to be seen regarding the reaction. Typically, these are used to tell us if a reaction is endothermic or exothermic, that is to say, is the system gaining energy or losing energy? Here's an example:

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2Fdownload%20(1).png?alt=media&token=5a9fcca7-a6e7-40db-a6c1-67b3f8f492ef

Image Courtesy of the University of Illinois

You can ignore "activation energy" for now, we'll get into that in the next section. What's important for you to understand is that in a reaction, energy is either released or absorbed and this will affect the energy involved in getting the reaction started.

The Progress of a Reaction

There are three main parts of a reaction: the reactants, the activated complex, the products. You've probably heard of reactants and products before, those being the stuff that goes in and comes out. However, the activated complex is the middle. Essentially, it's where a reaction is transitioning from reactants to products, and where bonds are not completely broken:

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2F3a02392d3cb54087cb6bb7f7f7270d57.png?alt=media&token=92d50354-633a-4078-90c9-26d2c4fcee97

Activation Energy and the Arrhenius Equation

What is Activation Energy?

Activation energy is actually quite simple - it is the energy required to break the bonds in a reaction to go from the reactants, to the activated complex, to the products. It is defined formally as "the energy difference between the reactants and the transition state" according to the College Board. On an energy diagram, this is shown by an arrow from the reactants to the peak of the graph, as you can see in the prior images.

The Arrhenius Equation

The Arrhenius equation relates the temperature dependence of the rate of an elementary reaction to the activation energy needed by molecular collisions to reach the transition state:

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2F47ef893163944b9b50fe4cb06bfbcc6d.png?alt=media&token=e229cb82-e0cd-4ded-af6f-96a951216c93

This equation can tell us how a rate constant changes based on changes in temperature. Note that for the AP exam, you will not have to use this equation to make calculations.

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ap chem study guides

โš›๏ธย  Unit 1: Atomic Structure and Properties

๐ŸŒ€ย  Unit 3: Intermolecular Forces and Properties

๐Ÿงชย  Unit 4: Chemical Reactions

๐Ÿ‘Ÿย  Unit 5: Kinetics

๐Ÿ”ฅย  Unit 6: Thermodynamics

โš–๏ธย  Unit 7: Equilibrium

ย  Unit 9: Applications of Thermodynamics

๐Ÿคบย  AP Chemistry Essentials

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