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AP Chemistry
7.10 Reaction Quotient and Le Châtelier’s Principle
7.9 Introduction to Le Châtelier’s Principle
7.3 Reaction Quotient and Equilibrium Constant
IntermediateMCQGraphicalProportional AnalysisConceptual20.3k
Create a grayscale line graph with a bare white plotting area and no gridlines. Label the horizontal axis “Time” and the vertical axis “Concentration (M).” Put y-axis tick marks at 0.100, 0.150, 0.200, and 0.225, and place a thin vertical marker labeled t₁ near the middle. Include a legend mapping a solid curve to NO₂ and a dashed curve to N₂O₄. Before the marker, both curves coincide as a horizontal segment at 0.100. At the marker, each curve makes an instantaneous vertical jump to 0.200. After the marker, the solid curve smoothly decreases and levels off at 0.150, while the dashed curve smoothly increases and levels off at 0.225. Both approach their final plateaus over the same time interval with no oscillation. Use uniform black strokes, clear axis arrowheads, and compact textbook proportions. No other curves, labels, text, shading, or annotations appear.
Concentrations before and after a sudden volume decrease
A sealed cylinder contains an equilibrium mixture represented by the equation

\(2\text{NO}_2\text{(g)} \rightleftharpoons \text{N}_2\text{O}_4\text{(g)}\)

At time \(t_1\), the volume of the cylinder is rapidly decreased to one-half its original value while the temperature remains constant. The concentrations are recorded in the graph.

Which statement best explains the concentration changes shown after \(t_1\)?

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