Chemical Kinetics — Chapter Summary
Tamil Nadu Board · Class 12 · Chemistry
Summary of Chemical Kinetics for Tamil Nadu Board Class 12 Chemistry. Part of the Tamil Nadu Board Class 12 Chemistry syllabus.
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Overview
Chemical kinetics is the branch of chemistry that studies the rates at which chemical reactions occur and the mechanisms by which they proceed. While thermodynamics tells us whether a reaction is feasible, kinetics answers the crucial question: How fast does a reaction happen? This chapter explores
Key Concepts
The rate of a reaction
The rate of a reaction is defined as the change in concentration of reactants or products per unit time. Mathematically, for a reaction A → B, the rat
Average rate is calculated over
Average rate is calculated over a longer time interval (Δt): Rate = -Δ[A]/Δt. It provides overall reaction speed but doesn't reveal how speed changes
The rate law expresses how reaction
The rate law expresses how reaction rate depends on reactant concentrations: Rate = k[A]ᵐ[B]ⁿ. Here, k is the rate constant (proportionality constant)
Reaction order is the sum
Reaction order is the sum of exponents in the rate law expression. For Rate = k[A]ᵐ[B]ⁿ, overall order = m + n. Orders can be zero, fractional, or int
Molecularity is the number of reactant
Molecularity is the number of reactant molecules involved in an elementary (single-step) reaction. It's assigned to individual steps in a reaction mec
Learning Objectives
- Define and calculate the rate of a chemical reaction using concentration changes
- Distinguish between average rate and instantaneous rate of a reaction
- Understand the relationship between rate law and reaction order
- Derive and apply integrated rate equations for zero and first-order reactions
- Calculate half-life periods and use them to determine reaction progress
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Sources & Official References
Content is aligned to the official syllabus. Refer to the board website for the latest curriculum.
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