Kinetics — A-Level Chemistry Revision
Revise Kinetics for A-Level Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel and OCR.
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Go to EquilibriumWhat is Kinetics?
Kinetics is the study of reaction rates and the factors that affect them, such as concentration, temperature, pressure, and catalysts. At A-Level, this involves determining the rate equation, rate constant (k), and order of reaction with respect to each reactant from experimental data. The Arrhenius equation is introduced to show the relationship between the rate constant and temperature, and reaction mechanisms are explored as a series of elementary steps that explain the overall observed kinetics.
Board notes: All boards require students to be able to determine rate equations from initial rates data. AQA often includes questions on the Arrhenius equation and calculating activation energy from graphical data. Edexcel may focus on the link between reaction mechanisms and the experimentally determined rate equation. OCR frequently tests the practical aspects of measuring reaction rates, such as colorimetry or gas collection.
Step-by-step explanationWorked example
For the reaction A + B -> C, the rate equation was found to be rate = k[A][B]^2. If the rate is 0.024 mol dm-3 s-1 when [A] = 0.1 mol dm-3 and [B] = 0.2 mol dm-3, calculate the rate constant, k. Step 1: Rearrange the rate equation to solve for k: k = rate / ([A][B]^2). Step 2: Substitute the values: k = 0.024 / (0.1 * (0.2)^2) = 0.024 / (0.1 * 0.04) = 6.0. Step 3: Determine the units: k = (mol dm-3 s-1) / ((mol dm-3)(mol dm-3)^2) = dm6 mol-2 s-1.
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Common mistakes
- 1Confusing the order of reaction with the stoichiometric coefficients in the balanced chemical equation. The order of reaction can only be determined experimentally.
- 2Incorrectly determining the units of the rate constant, k. The units depend on the overall order of the reaction and must be worked out for each specific rate equation.
- 3Misinterpreting concentration-time or rate-concentration graphs. For example, a straight line graph of concentration against time indicates a zero-order reaction, not a first-order one.
Kinetics exam questions
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Kinetics
Core concept
Kinetics is the study of reaction rates and the factors that affect them, such as concentration, temperature, pressure, and catalysts. At A-Level, this involves determining the rate equation, rate con…
Frequently asked questions
What is the role of a catalyst?
A catalyst increases the rate of a chemical reaction without being consumed in the process. It does this by providing an alternative reaction pathway with a lower activation energy, meaning more particles have sufficient energy to react upon collision.
What does the order of reaction actually mean?
The order of reaction with respect to a reactant tells you how the concentration of that reactant affects the rate. For example, if a reaction is second order with respect to reactant X, doubling the concentration of X will cause the rate to increase by a factor of 2^2, which is 4.