ThermalBreakdownTheory
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Catégorie :Category: nCreator TI-Nspire
Auteur Author: gurshan
Type : Classeur 3.0.1
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Mis en ligne Uploaded: 20/06/2025 - 05:51:39
Uploadeur Uploader: gurshan (Profil)
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Visibilité Visibility: Archive publique
Shortlink : https://tipla.net/a4738072
Type : Classeur 3.0.1
Page(s) : 1
Taille Size: 3.43 Ko KB
Mis en ligne Uploaded: 20/06/2025 - 05:51:39
Uploadeur Uploader: gurshan (Profil)
Téléchargements Downloads: 1
Visibilité Visibility: Archive publique
Shortlink : https://tipla.net/a4738072
Description
Fichier Nspire généré sur TI-Planet.org.
Compatible OS 3.0 et ultérieurs.
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1. Core Concepts and Definitions Quantity Symbol Units Description Temperature T K or °C Measure of average kinetic energy of particles Heat (Thermal Energy) Q J Energy transferred due to temperature difference Internal Energy U J Total KE + PE of particles in a system Specific Heat Capacity c J/kg·K Energy required to raise 1 kg of substance by 1 K Specific Latent Heat L J/kg Energy required for phase change of 1 kg of substance 2. Formulas and When to Use Them Heat energy transfer (no phase change) Q=mcT Use when an object is heating/cooling but not changing state. Phase change (no temperature change)Q=mLUse when an object melts, freezes, boils, or condenses. Thermal energy lost = thermal energy gainedQ lost =Q gainedIn calorimetry or mixing problems (no heat loss to surroundings). 3. Theory Breakdown Internal Energy (U) Sum of random KE and PE of particles KE depends on temperature PE depends on spacing and phase Temp increases internal energy increases Phase change internal energy increases (due to PE), but temperature stays the same Heat vs Temperature Heat = energy in transit (Q), flows from hot to cold Temperature = measure of average KE Objects at same temperature can have different heat content if their mass or specific heat differs Tricky MCQ: Which object contains more heat? Check mass × specific heat × temp, not just temperature. Specific Heat Capacity The amount of energy needed to raise 1 kg of a substance by 1°C (or K) Water has very high On MCQs, low c fast temp change; high c slow temp change (e.g., water heats up/cools down slowly) Specific Latent Heat Latent heat of fusion solid liquid (at melting point) Latent heat of vaporization liquid gas (at boiling point) During phase change: Temp stays constant Heat goes into breaking or forming bonds, i.e., PE change only Absolute Zero 0 K = point where particles have minimum internal energy Not zero energy, just zero KE (motion) No negative Kelvin possible 4. Ideal Gas Behavior A gas follows the ideal gas law: PV=nRTor T1 P 1 V 1 = T 2 P 2 V 2 (if n = const) Watch units:P = PaV = m³T = K C K: add 273.15 Molecular Model of Ideal Gas Assumptions:Random motion No intermolecular forces Elastic collisions Point particle KE T only Used to explain pressure, temperature, and volume changes microscopically 5. Graphs and Qualitative Reasoning Graph Behavior T vs Q (no phase change) Linear (slope = mc1) T vs Q (with phase change) Plateaus at phase change (Q increases, T constant) P vs V (isothermal) Hyperbola: PV=const P vs T (isochoric) Straight line: TP =constV vs T (isobaric) Linear: TV=const 6. High-Yield MCQ Traps Trap Question What to Remember Why is temp constant while boiling? Energy goes into breaking bonds (PE), not KE Which object has more thermal energy? Look at Q=mcT, not just T Gas is compressed rapidly. What happens? KE , so T , so P (use PV=nRT) Heat is added, but temp doesnt rise? Phase change is happening Why does metal heat faster than water? Lower c, so smaller energy needed per °C Which has highest avg KE? Highest temperature = highest avg KE (regardless of mass) Gas cooled, pressure dropped. Why? Fewer/less energetic collisions with container walls Strategy Summary Use Q=mcT for temp change, Q=mL for phase change If graph shows temp doesnt change, it's a phase change Convert °C K before using gas laws Watch units (V often in mL or L convert to m³!) Ideal gas assumption = no intermolecular forces Made with nCreator - tiplanet.org
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Compatible OS 3.0 et ultérieurs.
<<
1. Core Concepts and Definitions Quantity Symbol Units Description Temperature T K or °C Measure of average kinetic energy of particles Heat (Thermal Energy) Q J Energy transferred due to temperature difference Internal Energy U J Total KE + PE of particles in a system Specific Heat Capacity c J/kg·K Energy required to raise 1 kg of substance by 1 K Specific Latent Heat L J/kg Energy required for phase change of 1 kg of substance 2. Formulas and When to Use Them Heat energy transfer (no phase change) Q=mcT Use when an object is heating/cooling but not changing state. Phase change (no temperature change)Q=mLUse when an object melts, freezes, boils, or condenses. Thermal energy lost = thermal energy gainedQ lost =Q gainedIn calorimetry or mixing problems (no heat loss to surroundings). 3. Theory Breakdown Internal Energy (U) Sum of random KE and PE of particles KE depends on temperature PE depends on spacing and phase Temp increases internal energy increases Phase change internal energy increases (due to PE), but temperature stays the same Heat vs Temperature Heat = energy in transit (Q), flows from hot to cold Temperature = measure of average KE Objects at same temperature can have different heat content if their mass or specific heat differs Tricky MCQ: Which object contains more heat? Check mass × specific heat × temp, not just temperature. Specific Heat Capacity The amount of energy needed to raise 1 kg of a substance by 1°C (or K) Water has very high On MCQs, low c fast temp change; high c slow temp change (e.g., water heats up/cools down slowly) Specific Latent Heat Latent heat of fusion solid liquid (at melting point) Latent heat of vaporization liquid gas (at boiling point) During phase change: Temp stays constant Heat goes into breaking or forming bonds, i.e., PE change only Absolute Zero 0 K = point where particles have minimum internal energy Not zero energy, just zero KE (motion) No negative Kelvin possible 4. Ideal Gas Behavior A gas follows the ideal gas law: PV=nRTor T1 P 1 V 1 = T 2 P 2 V 2 (if n = const) Watch units:P = PaV = m³T = K C K: add 273.15 Molecular Model of Ideal Gas Assumptions:Random motion No intermolecular forces Elastic collisions Point particle KE T only Used to explain pressure, temperature, and volume changes microscopically 5. Graphs and Qualitative Reasoning Graph Behavior T vs Q (no phase change) Linear (slope = mc1) T vs Q (with phase change) Plateaus at phase change (Q increases, T constant) P vs V (isothermal) Hyperbola: PV=const P vs T (isochoric) Straight line: TP =constV vs T (isobaric) Linear: TV=const 6. High-Yield MCQ Traps Trap Question What to Remember Why is temp constant while boiling? Energy goes into breaking bonds (PE), not KE Which object has more thermal energy? Look at Q=mcT, not just T Gas is compressed rapidly. What happens? KE , so T , so P (use PV=nRT) Heat is added, but temp doesnt rise? Phase change is happening Why does metal heat faster than water? Lower c, so smaller energy needed per °C Which has highest avg KE? Highest temperature = highest avg KE (regardless of mass) Gas cooled, pressure dropped. Why? Fewer/less energetic collisions with container walls Strategy Summary Use Q=mcT for temp change, Q=mL for phase change If graph shows temp doesnt change, it's a phase change Convert °C K before using gas laws Watch units (V often in mL or L convert to m³!) Ideal gas assumption = no intermolecular forces Made with nCreator - tiplanet.org
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