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AP Chemistry
9.4 Thermodynamic and Kinetic Control
AdvancedMCQGraphicalConceptual22.7k
A reaction energy profile graph with bare axes and no gridlines. The horizontal x-axis is labeled Reaction Coordinate with an arrow pointing to the right. The vertical y-axis is labeled Gibbs Free Energy, \(G\), with an arrow pointing upward. A flat horizontal line segment on the left represents reactant \(\text{R}\) at an intermediate free energy level. Two curves emerge from \(\text{R}\). The first curve is a dashed line that rises to a moderate peak labeled \(\text{TS}_1\) and descends to a flat horizontal line segment labeled \(\text{P}_1\), positioned below the energy of \(\text{R}\). The second curve is a solid line that rises to a higher peak labeled \(\text{TS}_2\) (higher than \(\text{TS}_1\)) and descends to a flat horizontal line segment labeled \(\text{P}_2\), positioned below the energy of \(\text{P}_1\). No other particles, labels, text, or annotations appear.
Reaction coordinate diagram showing competing pathways from reactant \(\text{R}\) to products \(\text{P}_1\) and \(\text{P}_2\).
The reaction coordinate diagram below represents two competing pathways for the reaction of a single reactant, \(\text{R}\), to form either product \(\text{P}_1\) (dashed curve) or product \(\text{P}_2\) (solid curve).

When the reaction is carried out at \(200\text{ K}\), \(\text{P}_1\) is the predominant product formed. When the reaction is carried out at \(500\text{ K}\) and allowed to reach equilibrium, \(\text{P}_2\) is the predominant product in the mixture. Which of the following statements best explains these experimental observations based on the diagram?

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