Chemistry · Class 12 · Chapter 3
Chemical Kinetics
11 lessons 93 min 2 simulations
Thermodynamics says whether a reaction can go and equilibrium says how far; kinetics asks how fast, and why. The chapter defines average and instantaneous rates, writes rate laws from experiment, separates order (measured) from molecularity (a property of one elementary step), integrates the rate laws for zero- and first-order reactions to get concentration-time equations and half-lives, then explains why rates climb steeply with temperature (Arrhenius, activation energy, the energy distribution of molecules), how a catalyst opens an easier path, and what collision theory adds about energy and orientation.
What the exam asks
NEET tests rate expressions with stoichiometric coefficients, reading order from initial-rate tables, units of k for each order, zero- and first-order integrated equations and half-lives, 99% and 99.9% completion times, pseudo first order examples, the Arrhenius equation in its two-temperature log form, what a catalyst does and does not change, and the terms of collision theory. Marks go on forgetting to divide by the coefficient, mixing order with molecularity, using ln where the formula has log with 2.303, and forgetting that a zero-order half-life depends on the starting concentration.
Lessons
11 lessons · 93 min
1Rate of a reactionNCERT §3.17 min2Rate law and rate constantNCERT §3.2; §3.2.1; §3.2.27 min3Order of a reaction and units of kNCERT §3.2.36 min4Molecularity and mechanismNCERT §3.2.47 min5Zero-order reactionsNCERT §3.3; §3.3.17 min6First-order reactionsNCERT §3.3.26 min7Half-life and pseudo first orderNCERT §3.3.311 min 1 sim8Temperature and the Arrhenius equationNCERT §3.411 min 1 sim9Effect of a catalystNCERT §3.4.16 min10Collision theoryNCERT §3.57 min11Chapter reviewMust-know facts, traps and formulas18 min