AP®︎ Chemistry: Topic 5.1 Flashcards

Master key terms and definitions for Topic 5.1 of AP Chemistry – Reaction Rates to help you prep for quizzes and the AP exam.

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Term

Chemical Kinetics

Definition

The study of how fast reactions occur and what factors affect their speed.

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Chemical Kinetics
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The study of how fast reactions occur and what factors affect their speed.

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Reaction Rate
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The change in reactant or product concentration per unit time.

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Rate Expressions for Reactants and Products
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Rate = -Δ[reactant]/Δt or Δ[product]/Δt, with the negative sign for reactant loss.

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Units of Reaction Rate
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Usually mol L^-1 s^-1 or M/s, showing concentration change over time.

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Average Rate of Reaction
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The change in concentration over a finite time interval between two measured points.

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Instantaneous Rate of Reaction
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The rate at a specific moment, equal to the slope of the tangent line.

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Rate from a Concentration-Time Graph
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Find the slope of the curve; secant slope gives average rate, tangent slope gives instantaneous rate.

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Stoichiometric Relationships Between Rates
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Balanced coefficients relate species rates, so concentration changes occur in fixed mole ratios.

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Concentration and Reaction Rate
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Higher reactant concentration usually increases rate by causing more frequent effective collisions.

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Temperature and Reaction Rate
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Higher temperature usually increases rate because particles have greater average kinetic energy.

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Surface Area and Reaction Rate
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Greater exposed solid area usually increases rate by allowing more collisions at the surface.

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Catalyst
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A substance that speeds a reaction by providing an alternative pathway and is not consumed.

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Pressure and Reaction Rate for Gases
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Higher gas pressure usually increases rate by increasing particle concentration in a given volume.

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Rate of Disappearance and Rate of Appearance
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Reactants decrease while products increase, so their concentration changes have opposite signs.

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