Chapter 10 of 30
Concept Maps
Kinetic Theory of Gases — Concept Maps
NIOS · Class 12 · Physics
4 concept maps of Kinetic Theory of Gases for NIOS Class 12 Physics, each also written out as a text outline. Part of the NIOS Class 12 Physics syllabus.
44 questions37 flashcards20 formulas & key relations5 concepts
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4 Concept Maps
Kinetic Theory of Gases - Concept Hierarchy
The map in words
- Kinetic Theory of Gases
- Thermal Properties
- Heat Capacity
- Specific Heat
- Molar Heat
- Calorimetry
- Heat Transfer
- Principle
- Thermal Expansion
- Linear Alpha
- Areal Beta
- Volumetric Gamma
- Anomalous Water
- Heat Capacity
- Molecular Motion
- Assumptions
- Elastic Collisions
- Random Motion
- Negligible Forces
- Point Masses
- Pressure Derivation
- Momentum Change
- Collision Rate
- PV equation
- Temperature
- Kinetic Energy
- Boltzmann Constant
- Absolute Zero
- Assumptions
- Gas Laws
- Boyle's Law
- PV constant
- Charles's Law
- V proportional T
- Gay-Lussac's Law
- P proportional T
- Avogadro's Law
- Equal Molecules
- Dalton's Law
- Partial Pressures
- Graham's Law
- Diffusion Rate
- Boyle's Law
- Energy Distribution
- Degrees of Freedom
- Translational
- Rotational
- Vibrational
- Equipartition Law
- (1/2)kT per degree
- Heat Capacities
- Cv constant volume
- Cp constant pressure
- Cp - Cv = R
- Degrees of Freedom
- Thermal Properties
Kinetic Theory of Gases — Complete Chapter Overview
The map in words
- Kinetic Theory of Gases
- Thermal Properties
- Specific Heat C = dQ divided by m dT
- Calorimetry Heat Lost = Heat Gained
- Thermal Expansion
- Linear alpha
- Superficial beta = 2 alpha
- Cubical gamma = 3 alpha
- Anomalous Expansion of Water
- Max density at 4 degree C
- Assumptions of Kinetic Theory
- Large number of identical molecules
- Perfectly elastic collisions
- Negligible molecular size
- Straight line motion between collisions
- Negligible collision time
- Uniform distribution
- Pressure Derivation
- P = one third rho c squared
- PV = one third Mc squared
- Macroscopic meets Microscopic
- Kinetic Interpretation of Temperature
- Half m c squared = 3 by 2 kT
- k = Boltzmann Constant
- c rms = root of 3RT divided by M
- Absolute Zero means zero KE
- Gas Laws from Kinetic Theory
- Boyles Law PV = constant
- Charle Law V proportional T
- Gay Lussac Law P proportional T
- Avogadro Law N1 = N2
- Dalton Law P = P1 + P2 + P3
- Graham Law rate proportional 1 by root rho
- Degrees of Freedom
- Monoatomic f = 3
- Diatomic f = 5
- Triatomic f = 6
- Equipartition one half kT per DOF
- Specific Heats of Gases
- Cv at constant volume
- Cp at constant pressure
- Cp minus Cv = R
- Gamma = Cp divided by Cv
- Brownian Motion
- Random zig-zag motion
- Caused by molecular impacts
- Evidence for kinetic theory
- Mean Free Path sigma
- Thermal Properties
Kinetic Theory of Gases — Complete Concept Map
The map in words
- root（（Kinetic Theory
- of Gases））
- Thermal Concepts
- Specific Heat C
- Calorimetry
- Heat Lost = Heat Gained
- Thermal Expansion
- Alpha Linear
- Beta = 2Alpha Superficial
- Gamma = 3Alpha Cubical
- Anomalous Expansion
- Water densest at 4 Celsius
- Assumptions
- Random Identical Molecules
- Negligible Intermolecular Forces
- Size Negligible
- Straight Line Motion
- Elastic Collisions
- Uniform Distribution
- Pressure Derivation
- P = one-third rho c-squared
- PV = one-third N m c-squared
- Momentum Change = 2mu
- Temperature and KE
- KE = three-halves kT
- c-rms = root 3RT over M
- Boltzmann k = 1.38 x 10-23
- Gas Laws
- Boyle PV = constant
- Charles V proportional T
- Gay-Lussac P proportional T
- Avogadro Equal V Equal N
- Dalton P = P1 + P2 + P3
- Graham Rate = 1 over root rho
- Degrees of Freedom
- Monoatomic 3
- Diatomic 5
- Triatomic 6
- Equipartition half kT each
- Heat Capacities
- cv Constant Volume
- cp Constant Pressure
- cp - cv = R Mayer Relation
- Monoatomic cv = 3R over 2
- Diatomic cv = 5R over 2
- Brownian Motion
- Zigzag Random Path
- Due to Molecular Impacts
- Evidence for Kinetic Theory
- Mean Free Path
- sigma = 1 over root2 n pi d-squared
- Thermal Concepts
Kinetic Theory of Gases
The map in words
- Kinetic Theory of Gases
- Thermal Energy
- Assumptions of Kinetic Theory
- Gas Pressure Derivation
- Kinetic Interpretation of Temperature
- Gas Laws from Kinetic Theory
- Degrees of Freedom
- Law of Equipartition of Energy
- Heat Capacities of Gases
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Explore DiagramsFrequently Asked Questions
What are the important topics in Kinetic Theory of Gases for NIOS Class 12 Physics?
Key topics in Kinetic Theory of Gases include Thermal Energy: Heat Capacity and Specific Heat, Thermal Expansion: Linear, Superficial, and Cubical, Assumptions and Pressure of an Ideal Gas (Kinetic Theory), Kinetic Interpretation of Temperature and Mean Kinetic Energy. Study these first, then practise questions on each for the NIOS Class 12 board exam.
What do the concept maps for Kinetic Theory of Gases show?
The 4 maps show how the ideas in Kinetic Theory of Gases connect: Kinetic Theory of Gases - Concept Hierarchy; Kinetic Theory of Gases — Complete Chapter Overview. Each map is also written out as an outline on this page.
How should I revise Kinetic Theory of Gases for the NIOS Class 12 board exam?
Learn the core ideas first, then work through the 44 practice questions on Kinetic Theory of Gases. Revise definitions regularly and use flashcards for quick recall before the exam.
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Important Questions
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Formula Sheet
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Chapter Summary
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Study Plan
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Syllabus
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