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[
{
"slide": 1,
"fragments": [
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"fragment_index": -1,
"text_description": "Kinetic Theory\nFrom frenzied molecules to everyday pressure & temperature.",
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]
},
{
"slide": 2,
"fragments": [
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"fragment_index": -1,
"text_description": "Ideal Gas Model\nA hypothetical gas whose behaviour is fully described by the kinetic theory.\nCore assumptions:",
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"fragment_index": 1,
"text_description": "Ideal Gas",
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{
"fragment_index": 2,
"text_description": "Molecules are point-like; their own volume is negligible.",
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},
{
"fragment_index": 3,
"text_description": "They move randomly in straight lines between collisions.",
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},
{
"fragment_index": 4,
"text_description": "Collisions with walls and other molecules are perfectly elastic.",
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},
{
"fragment_index": 5,
"text_description": "No intermolecular forces act except during collisions.",
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},
{
"fragment_index": 6,
"text_description": "Which everyday gas comes closest to ideal behaviour at low pressure?",
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}
]
},
{
"slide": 3,
"fragments": [
{
"fragment_index": 1,
"text_description": "Collisions Build Pressure",
"image_description": ""
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{
"fragment_index": 2,
"text_description": "",
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{
"fragment_index": 3,
"text_description": "Origin of Gas Pressure",
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},
{
"fragment_index": 4,
"text_description": "When a molecule strikes the wall, its perpendicular velocity component reverses.",
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{
"fragment_index": 5,
"text_description": "The momentum change \\(\\Delta p = 2 m v_x\\) pushes the wall; countless such pushes per second create measurable pressure.",
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{
"fragment_index": 6,
"text_description": "Key Points:\nMomentum change per collision: \\(\\Delta p = 2 m v_x\\).\nForce equals total momentum transferred to the wall each second.\nMolecular pressure origin: many impacts distributed over the wall area.",
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}
]
},
{
"slide": 4,
"fragments": [
{
"fragment_index": -1,
"text_description": "Pressure Equation",
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{
"fragment_index": 1,
"text_description": "\\[ P = \\frac{1}{3} n m \\overline{v^{2}} \\]\nMicroscopically, pressure depends on how many molecules hit the walls and how hard they hit.",
"image_description": ""
},
{
"fragment_index": 2,
"text_description": "Variable Definitions\n\\(P\\)\nGas pressure (Pa)\n\\(n\\)\nNumber density (\\(\\text{m}^{-3}\\))\n\\(m\\)\nMass of one molecule (kg)\n\\( \\overline{v^{2}} \\)\nMean squared speed (\\(\\text{m}^{2}\\text{s}^{-2}\\))",
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},
{
"fragment_index": 3,
"text_description": "Applications\nIdeal Gas Law Link\nCombining with \\(PV = NkT\\) gives average kinetic energy \\( \\frac{3}{2}kT \\).\nTemperature–Pressure Relation\nIncreasing \\( \\overline{v^{2}} \\) with heat raises pressure at fixed volume.",
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}
]
},
{
"slide": 5,
"fragments": [
{
"fragment_index": -1,
"text_description": "Root-Mean-Square Speed",
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{
"fragment_index": 1,
"text_description": "1\n\\[PV = NkT\\]\nIdeal gas law relates macroscopic pressure and volume to particle number and absolute temperature.",
"image_description": ""
},
{
"fragment_index": 2,
"text_description": "2\n\\[P = \\frac{1}{3}\\frac{N m v_{\\text{rms}}^{2}}{V}\\]\nKinetic theory links pressure to the average translational kinetic energy of molecules.",
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},
{
"fragment_index": 3,
"text_description": "3\n\\[NkT = \\frac{1}{3} N m v_{\\text{rms}}^{2}\\]\nSubstitute step 2 into step 1 and cancel \\(V\\) to relate \\(T\\) to molecular speed.",
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},
{
"fragment_index": 4,
"text_description": "4\n\\[v_{\\text{rms}} = \\sqrt{\\frac{3kT}{m}}\\]\nSolving shows root-mean-square speed rises with temperature and falls with molecular mass.",
"image_description": ""
},
{
"fragment_index": 5,
"text_description": "Key Insight:\nTemperature is a direct measure of the average kinetic energy of gas particles; higher \\(T\\) means faster molecules.",
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}
]
},
{
"slide": 6,
"fragments": [
{
"fragment_index": -1,
"text_description": "Real vs Ideal Gas",
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{
"fragment_index": 1,
"text_description": "Fig 12.1 Compressibility factor Z vs pressure",
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"fragment_index": 2,
"text_description": "Reading Fig 12.1\nThe flat line at \\(Z = 1\\) shows an ideal gas.\nReal gas curves peel away at high pressure or low temperature because intermolecular forces and molecular volume matter.\nKey Points:\nDeviation is negligible at low pressure.\nHigh temperature reduces attractive forces, giving ideality.\nUse ideal gas law only under these conditions.",
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}
]
},
{
"slide": 7,
"fragments": []
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{
"slide": 8,
"fragments": [
{
"fragment_index": -1,
"text_description": "Multiple Choice Question\nCorrect!\nSince \\( \\overline{E_k} \\propto T \\), doubling \\(T\\) doubles the average kinetic energy.\nIncorrect\nRemember, average kinetic energy varies linearly with absolute temperature.\nconst correctOption = 0;\n const answerCards = document.querySelectorAll('.answer-card');\n const submitBtn = document.getElementById('submitBtn');\n const feedbackCorrect = document.getElementById('feedbackCorrect');\n const feedbackIncorrect = document.getElementById('feedbackIncorrect');\n\n let selectedOption = null;\n\n answerCards.forEach((card, index) => {\n card.addEventListener('click', () => {\n answerCards.forEach(c => c.classList.remove('border-blue-500', 'bg-blue-50', 'animate-shake'));\n card.classList.add('border-blue-500', 'bg-blue-50');\n selectedOption = index;\n });\n });\n\n submitBtn.addEventListener('click', () => {\n if (selectedOption === null) return;\n\n if (selectedOption === correctOption) {\n feedbackCorrect.classList.remove('hidden');\n feedbackIncorrect.classList.add('hidden');\n } else {\n feedbackIncorrect.classList.remove('hidden');\n feedbackCorrect.classList.add('hidden');\n answerCards[selectedOption].classList.add('animate-shake');\n }\n });",
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"fragment_index": 1,
"text_description": "Question\nFor an ideal gas, if the absolute temperature \\(T\\) is doubled, what happens to the average translational kinetic energy of its molecules?",
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},
{
"fragment_index": 2,
"text_description": "1\nIt doubles",
"image_description": ""
},
{
"fragment_index": 3,
"text_description": "2\nIt becomes half",
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},
{
"fragment_index": 4,
"text_description": "3\nIt becomes four times",
"image_description": ""
},
{
"fragment_index": 5,
"text_description": "4\nIt remains unchanged",
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},
{
"fragment_index": 6,
"text_description": "Hint:\nUse \\( \\overline{E_k} = \\frac{3}{2} k T \\). Average kinetic energy is directly proportional to absolute temperature.",
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},
{
"fragment_index": 7,
"text_description": "Submit Answer",
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}
]
},
{
"slide": 9,
"fragments": [
{
"fragment_index": -1,
"text_description": "Key Takeaways",
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{
"fragment_index": 1,
"text_description": "Molecular Motion (Recap)\nRapid, random molecular collisions with walls create pressure—foundation of microscopic gas view.",
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{
"fragment_index": 2,
"text_description": "Temperature = Energy\nGas temperature directly reflects average translational kinetic energy per molecule.",
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},
{
"fragment_index": 3,
"text_description": "Micro-Macro Bridge\n\\(P = \\frac{1}{3} n m v^{2}\\) mathematically links particle motion to measurable pressure.",
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},
{
"fragment_index": 4,
"text_description": "Ideal Gas Limit\nPoint particles with no forces obey \\(PV = nRT\\), unifying motion and macroscopic law.",
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},
{
"fragment_index": 5,
"text_description": "Real-Gas Deviations\nDepartures highlight intermolecular attractions and sizes, sharpening our microscopic understanding.",
"image_description": ""
}
]
}
]