Draw a graph showing the reaction pathway for an overall exothermic reaction with two intermediates that are produced at different rates. On your graph, indicate the reactants, products, intermediates, transition states, and activation energies. [Sections 14.6 and 14.7]
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Step 1: Begin by drawing the x-axis and y-axis on your graph. The x-axis will represent the reaction coordinate, which is the progress of the reaction from reactants to products. The y-axis will represent the potential energy of the system.
Step 2: Plot the starting point of the graph at a higher energy level to represent the reactants. Label this point as 'Reactants'.
Step 3: Draw a curve that rises to a peak, representing the first transition state. This peak is the activation energy for the first step of the reaction. Label this peak as 'Transition State 1'.
Step 4: After the first transition state, the curve should drop to a lower energy level than the reactants, indicating the formation of the first intermediate. Label this point as 'Intermediate 1'.
Step 5: Repeat the process for the second intermediate and transition state. Draw another curve rising to a second peak (Transition State 2) and then dropping to a lower energy level than Intermediate 1, indicating the formation of the second intermediate. Finally, the curve should drop further to the lowest energy level, representing the products. Label this final point as 'Products'.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Exothermic Reactions
Exothermic reactions are chemical processes that release energy, usually in the form of heat, to the surroundings. This occurs when the total energy of the products is lower than that of the reactants, resulting in a negative change in enthalpy (ΔH < 0). Understanding this concept is crucial for interpreting the energy changes depicted in reaction pathway graphs.
Reaction intermediates are transient species formed during the conversion of reactants to products. They exist for a limited time and are not present in the final products. In the context of the question, recognizing the role of intermediates is essential for accurately representing their formation and decay on the reaction pathway graph.
Activation energy is the minimum energy required for a reaction to occur, which corresponds to the energy barrier that must be overcome to reach the transition state. The transition state is a high-energy configuration of atoms that occurs during the transformation from reactants to products. Understanding these concepts is vital for illustrating the energy profile of the reaction, including the heights of the activation energy barriers associated with each step.
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