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AP Chemistry
9.4 Thermodynamic and Kinetic Control
AdvancedMCQDrawing RepresentationsConceptual16.4k
A grayscale reaction energy profile with a vertical axis labeled 'Gibbs Free Energy, \(G\)' and a horizontal axis labeled 'Reaction Coordinate'. Both axes have arrows indicating increasing direction; no gridlines appear. At the far left, a horizontal plateau represents the initial state labeled '\(\text{R}\)'. From '\(\text{R}\)', two smooth curves split into competing reaction pathways. The first curve, drawn with a dashed line, ascends to a lower peak labeled '\(\text{TS}_1\)' and descends to a horizontal plateau labeled '\(\text{X}\)' that lies below '\(\text{R}\)'. The second curve, drawn with a solid line, ascends to a higher peak labeled '\(\text{TS}_2\)' and descends to a horizontal plateau labeled '\(\text{Y}\)' that lies substantially lower than both '\(\text{R}\)' and '\(\text{X}\)'. A legend in the upper-right corner indicates: dashed line = Pathway to \(\text{X}\), solid line = Pathway to \(\text{Y}\). No other curves, gridlines, labels, or annotations appear.
Reaction energy profile for the conversion of \(\text{R(g)}\) to \(\text{X(g)}\) and \(\text{Y(g)}\).
The reaction energy profile below represents two competing pathways for the conversion of reactant \(\text{R(g)}\) into products \(\text{X(g)}\) and \(\text{Y(g)}\).

An experiment is conducted in which \(\text{R(g)}\) is allowed to react at \(200\text{ K}\), yielding predominantly \(\text{X(g)}\). When the reaction is carried out at \(500\text{ K}\) and given sufficient time to reach chemical equilibrium, \(\text{Y(g)}\) is found to be the predominant product.

Which of the following statements is best supported by the diagram and the experimental observations?

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