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AP Chemistry
9.4 Thermodynamic and Kinetic Control
AdvancedMCQGraphicalConceptual21.7k
A reaction energy profile graph is displayed on bare vertical and horizontal axes without gridlines. The vertical axis is labeled Gibbs Free Energy, G. The horizontal axis is labeled Reaction Coordinate. A single horizontal plateau labeled R is located at an intermediate energy level on the left. Two curves originate from R and branch to the right. Pathway 1 is drawn as a solid black curve that rises to a transition state peak labeled TS1 and then descends to a product plateau labeled P1 located below the energy level of R. Pathway 2 is drawn as a dashed black curve that rises to a transition state peak labeled TS2, positioned significantly higher than TS1, and then descends to a product plateau labeled P2 located significantly lower in energy than both R and P1. A legend in the upper right corner indicates: solid line = Pathway 1, dashed line = Pathway 2. No other particles, labels, text, or annotations appear.
Gibbs free energy profile for competing pathways converting reactant \(\text{R}\) into \(\text{P}_1\) and \(\text{P}_2\).
The reaction energy profile for the conversion of reactant \(\text{R}\) into two different isomeric products, \(\text{P}_1\) and \(\text{P}_2\), along competing elementary pathways is shown in the diagram.

A sample of \(\text{R}\) is reacted under Condition X (\(200\text{ K}\) for a short reaction time, followed by rapid cooling). A separate sample of \(\text{R}\) is reacted under Condition Y (\(550\text{ K}\) for an extended period until chemical equilibrium is established).

Based on the energy profile, which of the following identifies the predominant product formed under each condition and provides the best justification?

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