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  "events": [ {
    "tStartMs": 6875,
    "dDurationMs": 3578,
    "segs": [ {
      "utf8": "There's a concept that's crucial\nto chemistry and physics."
    } ]
  }, {
    "tStartMs": 10453,
    "dDurationMs": 4840,
    "segs": [ {
      "utf8": "It helps explain why physical processes\ngo one way and not the other:"
    } ]
  }, {
    "tStartMs": 15293,
    "dDurationMs": 1556,
    "segs": [ {
      "utf8": "why ice melts,"
    } ]
  }, {
    "tStartMs": 16849,
    "dDurationMs": 2430,
    "segs": [ {
      "utf8": "why cream spreads in coffee,"
    } ]
  }, {
    "tStartMs": 19279,
    "dDurationMs": 3250,
    "segs": [ {
      "utf8": "why air leaks out of a punctured tire."
    } ]
  }, {
    "tStartMs": 22529,
    "dDurationMs": 4510,
    "segs": [ {
      "utf8": "It's entropy, and it's notoriously\ndifficult to wrap our heads around."
    } ]
  }, {
    "tStartMs": 27039,
    "dDurationMs": 4840,
    "segs": [ {
      "utf8": "Entropy is often described as\na measurement of disorder."
    } ]
  }, {
    "tStartMs": 31879,
    "dDurationMs": 3860,
    "segs": [ {
      "utf8": "That's a convenient image,\nbut it's unfortunately misleading."
    } ]
  }, {
    "tStartMs": 35739,
    "dDurationMs": 2772,
    "segs": [ {
      "utf8": "For example, which is more disordered -"
    } ]
  }, {
    "tStartMs": 38511,
    "dDurationMs": 4958,
    "segs": [ {
      "utf8": "a cup of crushed ice or a glass\nof room temperature water?"
    } ]
  }, {
    "tStartMs": 43469,
    "dDurationMs": 1904,
    "segs": [ {
      "utf8": "Most people would say the ice,"
    } ]
  }, {
    "tStartMs": 45373,
    "dDurationMs": 3696,
    "segs": [ {
      "utf8": "but that actually has lower entropy."
    } ]
  }, {
    "tStartMs": 49069,
    "dDurationMs": 3829,
    "segs": [ {
      "utf8": "So here's another way of thinking\nabout it through probability."
    } ]
  }, {
    "tStartMs": 52898,
    "dDurationMs": 4392,
    "segs": [ {
      "utf8": "This may be trickier to understand,\nbut take the time to internalize it"
    } ]
  }, {
    "tStartMs": 57290,
    "dDurationMs": 3970,
    "segs": [ {
      "utf8": "and you'll have a much better \nunderstanding of entropy."
    } ]
  }, {
    "tStartMs": 61260,
    "dDurationMs": 2401,
    "segs": [ {
      "utf8": "Consider two small solids"
    } ]
  }, {
    "tStartMs": 63661,
    "dDurationMs": 3880,
    "segs": [ {
      "utf8": "which are comprised \nof six atomic bonds each."
    } ]
  }, {
    "tStartMs": 67541,
    "dDurationMs": 5240,
    "segs": [ {
      "utf8": "In this model, the energy in each solid\nis stored in the bonds."
    } ]
  }, {
    "tStartMs": 72781,
    "dDurationMs": 2511,
    "segs": [ {
      "utf8": "Those can be thought of \nas simple containers,"
    } ]
  }, {
    "tStartMs": 75292,
    "dDurationMs": 4778,
    "segs": [ {
      "utf8": "which can hold indivisible units of energy\nknown as quanta."
    } ]
  }, {
    "tStartMs": 80070,
    "dDurationMs": 4531,
    "segs": [ {
      "utf8": "The more energy a solid has,\nthe hotter it is."
    } ]
  }, {
    "tStartMs": 84601,
    "dDurationMs": 4441,
    "segs": [ {
      "utf8": "It turns out that there are numerous\nways that the energy can be distributed"
    } ]
  }, {
    "tStartMs": 89042,
    "dDurationMs": 1510,
    "segs": [ {
      "utf8": "in the two solids"
    } ]
  }, {
    "tStartMs": 90552,
    "dDurationMs": 4040,
    "segs": [ {
      "utf8": "and still have the same \ntotal energy in each."
    } ]
  }, {
    "tStartMs": 94592,
    "dDurationMs": 3910,
    "segs": [ {
      "utf8": "Each of these options \nis called a microstate."
    } ]
  }, {
    "tStartMs": 98502,
    "dDurationMs": 4839,
    "segs": [ {
      "utf8": "For six quanta of energy in Solid A\nand two in Solid B,"
    } ]
  }, {
    "tStartMs": 103341,
    "dDurationMs": 4491,
    "segs": [ {
      "utf8": "there are 9,702 microstates."
    } ]
  }, {
    "tStartMs": 107832,
    "dDurationMs": 5029,
    "segs": [ {
      "utf8": "Of course, there are other ways our eight\nquanta of energy can be arranged."
    } ]
  }, {
    "tStartMs": 112861,
    "dDurationMs": 4972,
    "segs": [ {
      "utf8": "For example, all of the energy\ncould be in Solid A and none in B,"
    } ]
  }, {
    "tStartMs": 117833,
    "dDurationMs": 3039,
    "segs": [ {
      "utf8": "or half in A and half in B."
    } ]
  }, {
    "tStartMs": 120872,
    "dDurationMs": 3282,
    "segs": [ {
      "utf8": "If we assume that each microstate\nis equally likely,"
    } ]
  }, {
    "tStartMs": 124154,
    "dDurationMs": 2640,
    "segs": [ {
      "utf8": "we can see that some of the energy\nconfigurations"
    } ]
  }, {
    "tStartMs": 126794,
    "dDurationMs": 3749,
    "segs": [ {
      "utf8": "have a higher probability of occurring\nthan others."
    } ]
  }, {
    "tStartMs": 130543,
    "dDurationMs": 3641,
    "segs": [ {
      "utf8": "That's due to their greater number\nof microstates."
    } ]
  }, {
    "tStartMs": 134184,
    "dDurationMs": 5959,
    "segs": [ {
      "utf8": "Entropy is a direct measure of each\nenergy configuration's probability."
    } ]
  }, {
    "tStartMs": 140143,
    "dDurationMs": 3050,
    "segs": [ {
      "utf8": "What we see is that the energy\nconfiguration"
    } ]
  }, {
    "tStartMs": 143193,
    "dDurationMs": 3650,
    "segs": [ {
      "utf8": "in which the energy\nis most spread out between the solids"
    } ]
  }, {
    "tStartMs": 146843,
    "dDurationMs": 2081,
    "segs": [ {
      "utf8": "has the highest entropy."
    } ]
  }, {
    "tStartMs": 148924,
    "dDurationMs": 1550,
    "segs": [ {
      "utf8": "So in a general sense,"
    } ]
  }, {
    "tStartMs": 150474,
    "dDurationMs": 4379,
    "segs": [ {
      "utf8": "entropy can be thought of as a measurement\nof this energy spread."
    } ]
  }, {
    "tStartMs": 154853,
    "dDurationMs": 3040,
    "segs": [ {
      "utf8": "Low entropy means \nthe energy is concentrated."
    } ]
  }, {
    "tStartMs": 157893,
    "dDurationMs": 3730,
    "segs": [ {
      "utf8": "High entropy means it's spread out."
    } ]
  }, {
    "tStartMs": 161623,
    "dDurationMs": 4142,
    "segs": [ {
      "utf8": "To see why entropy is useful for\nexplaining spontaneous processes,"
    } ]
  }, {
    "tStartMs": 165765,
    "dDurationMs": 2310,
    "segs": [ {
      "utf8": "like hot objects cooling down,"
    } ]
  }, {
    "tStartMs": 168075,
    "dDurationMs": 4359,
    "segs": [ {
      "utf8": "we need to look at a dynamic system\nwhere the energy moves."
    } ]
  }, {
    "tStartMs": 172434,
    "dDurationMs": 2501,
    "segs": [ {
      "utf8": "In reality, energy doesn't stay put."
    } ]
  }, {
    "tStartMs": 174935,
    "dDurationMs": 3130,
    "segs": [ {
      "utf8": "It continuously moves between \nneighboring bonds."
    } ]
  }, {
    "tStartMs": 178065,
    "dDurationMs": 2141,
    "segs": [ {
      "utf8": "As the energy moves,"
    } ]
  }, {
    "tStartMs": 180206,
    "dDurationMs": 2749,
    "segs": [ {
      "utf8": "the energy configuration can change."
    } ]
  }, {
    "tStartMs": 182955,
    "dDurationMs": 2130,
    "segs": [ {
      "utf8": "Because of the distribution \nof microstates,"
    } ]
  }, {
    "tStartMs": 185085,
    "dDurationMs": 4751,
    "segs": [ {
      "utf8": "there's a 21% chance that the system\nwill later be in the configuration"
    } ]
  }, {
    "tStartMs": 189836,
    "dDurationMs": 3759,
    "segs": [ {
      "utf8": "in which the energy is maximally \nspread out,"
    } ]
  }, {
    "tStartMs": 193595,
    "dDurationMs": 3762,
    "segs": [ {
      "utf8": "there's a 13% chance that it will\nreturn to its starting point,"
    } ]
  }, {
    "tStartMs": 197357,
    "dDurationMs": 5500,
    "segs": [ {
      "utf8": "and an 8% chance that A will actually\ngain energy."
    } ]
  }, {
    "tStartMs": 202857,
    "dDurationMs": 4078,
    "segs": [ {
      "utf8": "Again, we see that because there are\nmore ways to have dispersed energy"
    } ]
  }, {
    "tStartMs": 206935,
    "dDurationMs": 3091,
    "segs": [ {
      "utf8": "and high entropy than concentrated energy,"
    } ]
  }, {
    "tStartMs": 210026,
    "dDurationMs": 2532,
    "segs": [ {
      "utf8": "the energy tends to spread out."
    } ]
  }, {
    "tStartMs": 212558,
    "dDurationMs": 2951,
    "segs": [ {
      "utf8": "That's why if you put a hot object\nnext to a cold one,"
    } ]
  }, {
    "tStartMs": 215509,
    "dDurationMs": 4911,
    "segs": [ {
      "utf8": "the cold one will warm up\nand the hot one will cool down."
    } ]
  }, {
    "tStartMs": 220420,
    "dDurationMs": 1447,
    "segs": [ {
      "utf8": "But even in that example,"
    } ]
  }, {
    "tStartMs": 221867,
    "dDurationMs": 5249,
    "segs": [ {
      "utf8": "there is an 8% chance that the hot object\nwould get hotter."
    } ]
  }, {
    "tStartMs": 227116,
    "dDurationMs": 4311,
    "segs": [ {
      "utf8": "Why doesn't this ever happen\nin real life?"
    } ]
  }, {
    "tStartMs": 231427,
    "dDurationMs": 2750,
    "segs": [ {
      "utf8": "It's all about the size of the system."
    } ]
  }, {
    "tStartMs": 234177,
    "dDurationMs": 3880,
    "segs": [ {
      "utf8": "Our hypothetical solids only had\nsix bonds each."
    } ]
  }, {
    "tStartMs": 238057,
    "dDurationMs": 5881,
    "segs": [ {
      "utf8": "Let's scale the solids up to 6,000 bonds\nand 8,000 units of energy,"
    } ]
  }, {
    "tStartMs": 243938,
    "dDurationMs": 3589,
    "segs": [ {
      "utf8": "and again start the system with\nthree-quarters of the energy in A"
    } ]
  }, {
    "tStartMs": 247527,
    "dDurationMs": 2600,
    "segs": [ {
      "utf8": "and one-quarter in B."
    } ]
  }, {
    "tStartMs": 250127,
    "dDurationMs": 4210,
    "segs": [ {
      "utf8": "Now we find that chance of A\nspontaneously acquiring more energy"
    } ]
  }, {
    "tStartMs": 254337,
    "dDurationMs": 2910,
    "segs": [ {
      "utf8": "is this tiny number."
    } ]
  }, {
    "tStartMs": 257247,
    "dDurationMs": 5061,
    "segs": [ {
      "utf8": "Familiar, everyday objects have many, many\ntimes more particles than this."
    } ]
  }, {
    "tStartMs": 262308,
    "dDurationMs": 3612,
    "segs": [ {
      "utf8": "The chance of a hot object \nin the real world getting hotter"
    } ]
  }, {
    "tStartMs": 265920,
    "dDurationMs": 2091,
    "segs": [ {
      "utf8": "is so absurdly small,"
    } ]
  }, {
    "tStartMs": 268011,
    "dDurationMs": 2398,
    "segs": [ {
      "utf8": "it just never happens."
    } ]
  }, {
    "tStartMs": 270409,
    "dDurationMs": 1119,
    "segs": [ {
      "utf8": "Ice melts,"
    } ]
  }, {
    "tStartMs": 271528,
    "dDurationMs": 1390,
    "segs": [ {
      "utf8": "cream mixes in,"
    } ]
  }, {
    "tStartMs": 272918,
    "dDurationMs": 1758,
    "segs": [ {
      "utf8": "and tires deflate"
    } ]
  }, {
    "tStartMs": 274676,
    "dDurationMs": 5266,
    "segs": [ {
      "utf8": "because these states have more\ndispersed energy than the originals."
    } ]
  }, {
    "tStartMs": 279942,
    "dDurationMs": 3688,
    "segs": [ {
      "utf8": "There's no mysterious force\nnudging the system towards higher entropy."
    } ]
  }, {
    "tStartMs": 283630,
    "dDurationMs": 5298,
    "segs": [ {
      "utf8": "It's just that higher entropy is always\nstatistically more likely."
    } ]
  }, {
    "tStartMs": 288928,
    "dDurationMs": 3552,
    "segs": [ {
      "utf8": "That's why entropy has been called\ntime's arrow."
    } ]
  }, {
    "tStartMs": 292480,
    "dDurationMs": 4259,
    "segs": [ {
      "utf8": "If energy has the opportunity\nto spread out, it will."
    } ]
  } ]
}