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AP Chemistry
3.5 Kinetic Molecular Theory
3.4 Ideal Gas Law
IntermediateMCQDrawing RepresentationsConceptual20k
A two-panel grayscale diagram titled State 1 and State 2. A legend indicates: open circle = gas particle, straight arrow = particle velocity vector. State 1 shows a tall rectangular cylinder of volume \(2.0\text{ L}\) with a horizontal piston near the top. Inside State 1, there are exactly 6 open circles evenly distributed; each circle has an attached straight arrow of uniform length \(1.0\text{ cm}\) pointing in random directions. State 2 shows the identical cylinder with the piston positioned at half the original height, enclosing a volume of \(1.0\text{ L}\). Inside State 2, there are exactly 6 open circles evenly distributed in the smaller space; each circle has an attached straight arrow of the same uniform length \(1.0\text{ cm}\) pointing in random directions. The cylinder walls and piston are drawn with solid black lines. No other particles, labels, text, or annotations appear.
Particulate representations of the gas sample at \(298\text{ K}\) before and after compression.
A sample of an ideal gas is confined in a rigid-walled cylinder fitted with a movable piston at a constant temperature of \(298\text{ K}\). The piston is slowly pushed downward, decreasing the volume of the gas from \(2.0\text{ L}\) (State 1) to \(1.0\text{ L}\) (State 2), as represented in the diagrams below.

Based on the representations and the principles of kinetic molecular theory, which of the following best explains why the pressure exerted by the gas in State 2 is greater than the pressure in State 1?

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