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AP Chemistry
9.4 Thermodynamic and Kinetic Control
AdvancedMCQConceptualExperimental18.2k
A reaction energy profile graph plotted on bare axes without gridlines. The vertical axis is labeled Potential Energy (kJ/mol) and the horizontal axis is labeled Reaction Coordinate. A horizontal reactant plateau at 0 kJ/mol is labeled R. A solid curve for Pathway to X rises from R to an activation barrier peak at 40 kJ/mol, then descends to a product plateau at -15 kJ/mol labeled X. A dashed curve for Pathway to Y rises from R to an activation barrier peak at 85 kJ/mol, then descends to a lower product plateau at -60 kJ/mol labeled Y. A legend in the upper-right corner contains two entries: a solid line labeled Pathway to X and a dashed line labeled Pathway to Y. No other lines, curves, labels, or annotations appear.
Reaction energy profile for the competing pathways from reactant \(\text{R}\) to products \(\text{X}\) and \(\text{Y}\).
A chemist investigates the reaction of reactant \(\text{R}\), which can follow two competing pathways to yield either product \(\text{X}\) or product \(\text{Y}\), as represented in the reaction energy profile below.

When the reaction is carried out at \(200\text{ K}\) for a brief duration, product \(\text{X}\) is the major product formed. When the reaction is instead carried out at \(500\text{ K}\) and allowed to reach dynamic equilibrium, product \(\text{Y}\) is the major product. Which of the following statements best explains why product \(\text{Y}\) predominates at \(500\text{ K}\)?

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