Question

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
AB + CD → AD + BC AB + CD 10 kJ 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 following 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.

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 of negative. There should be a conclusion statement for each graph.


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Answer 1

Potential energy diagrams are used to represent the energy changes in a chemical reaction. Endothermic reactions have an uphill energy curve and absorb energy, while exothermic reactions have a downhill energy curve and release energy. The sign of the enthalpy change indicates if the reaction is endothermic or exothermic.

Step-by-step explanation:

Potential energy diagrams are used to represent the energy changes that occur during a chemical reaction. By plotting the potential energy on the y-axis and the reaction progress on the x-axis, these diagrams show the change in potential energy as reactants are converted into products.

An endothermic reaction is represented by an uphill energy curve, where the reactants have lower potential energy than the products. This indicates that the reaction absorbs energy from its surroundings. An exothermic reaction, on the other hand, is represented by a downhill energy curve, where the reactants have higher potential energy than the products. This indicates that the reaction releases energy to its surroundings.

The sign of the enthalpy change (ΔH) is positive for an endothermic reaction and negative for an exothermic reaction. This reflects the energy flow in the reaction, with endothermic reactions absorbing energy from the surroundings and exothermic reactions releasing energy to the surroundings.