Chemistry · Class 12 · Chapter 3

Chemical Kinetics

11 lessons111 min8 simulations10 practice questions

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.

Also called: rate of reaction · order of reaction · rate law · activation energy

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Lessons

11 lessons · 111 min

01Rate of a reactionNCERT §3.110 min1 sim 02Rate law and rate constantNCERT §3.2; §3.2.1; §3.2.210 min1 sim 03Order of a reaction and units of kNCERT §3.2.36 min 04Molecularity and mechanismNCERT §3.2.47 min 05Zero-order reactionsNCERT §3.3; §3.3.17 min 06First-order reactionsNCERT §3.3.29 min1 sim 07Half-life and pseudo first orderNCERT §3.3.314 min2 sims 08Temperature and the Arrhenius equationNCERT §3.411 min1 sim 09Effect of a catalystNCERT §3.4.19 min1 sim 10Collision theoryNCERT §3.510 min1 sim 11Chapter reviewMust-know facts, traps and formulas18 min

Simulations

8 in this chapter

One reaction, three rates?In: Rate of a reaction Can you find a rate law from initial rates alone?In: Rate law and rate constant Which plot turns the data into a straight line?In: First-order reactions How does a reactant run out: steadily or by halves?In: Half-life and pseudo first order Do half-lives shrink, stay or grow?In: Half-life and pseudo first order Why does a little heat speed a reaction so much?In: Temperature and the Arrhenius equation What does a catalyst change, and what does it leave alone?In: Effect of a catalyst Is a hard enough collision always enough?In: Collision theory