Endothermic and Exothermic Activity



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Endothermic and Exothermic Activity
For this assignment, you will create your own potential energy diagrams for each of the three chemical reactions. Then you will analyze the data and your diagrams for each reaction.
Generic Reactions
Reactants
Products
Transition State
Synthesis
A + B AB
A + B | -15 kJ
AB | 20 kJ
30 kJ
Single Replacement
C + AB CB + A
C + AB | 65 kJ
CB + A | 30 kJ
85 kJ
Double Replacement
ABf + CD AD + BC
AB + CD | 10 k
AD + BC | 60 kJ
75 kJ
To assist you, use the enthalpy values in the data chart for each generic reaction provided. Be sure to follow the summary of steps below.
* Illustrate the x- and y-axes to show the reaction pathway and potential energy, in kilojoules.
Ensure your energy intervals are appropriate for the data.
* Plot the enthalpy values of the reactants, products, and transition state using three horizontal dotted lines across the graph for each.
* Draw the energy curve from the reactants line to the transition state and curve the line back down to the energy of the products. Label the reactants, products, and transition state.
* Illustrate double-headed arrows to represent both the total change in enthalpy (ΔH) and the activation energy (Ea).
* Calculate the total change in enthalpy and the activation energy using the energy values provided for each reaction. Record those values below the graph.
* Make sure correct units are included.

Activation Energy: 45 kJ
Enthalpy change: +35 kJ
This diagram shows the change between the product and reactant. Also, because the reactant’s potential energy is higher than the product. This shows that heat was released.
Also, because energy was lost, the enthalpy is negative.

Activation Energy: 20 kJ
Enthalpy change: -35 kJ
Due to the diagram show the reactant’s potential energy is higher than the product’s, heat is released. Since potential energy is lost, the enthalpy is negative. Also the diagram uses the variation between the product and reactant to determine whether it is endothermic or exothermic.

Activation Energy: 65 kJ
Enthalpy change: +50 kJ
The heat is absorbed due to the potential energy of the product being higher than the reactant, which shows heat was gained. Also due to the gained potential energy, the enthalpy is positive.
Seeing the difference between the product and reactant can be used to find out whether it is endothermic or exothermic.
Conclusion Statement
Write a two to four sentence conclusion statement explaining how the potential energy diagram is used to identify if the reaction is endothermic or exothermic, if heat was released or absorbed, and why the sign of enthalpy change was positive or negative. There should be a conclusion statement for each graph.


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