Use the second law of thermodynamics to explain briefly what happens, in terms of the entropy...

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Chemistry

Use the second law of thermodynamics to explain briefly whathappens, in terms of the entropy of the stable phase, when thetemperature of ice is raised from -10 Â°C to 10 Â°C.

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what does all that energy spreading out have to do withentropyEntropy change is a measure of the molecular motional energyplus any phase change energy that has been dispersed in a systemat a specific temperatureAlwaysmotional energy flows in the direction of hotter to coolerbecause that direction of dispersal results in agreater amount of spreading out of energy than the reverse Entropychange qrevT quantitatively measures energydispersingspreading out Its profound importance is that it alwaysincreases in a hotter to cooler process so long as you considerthe universe of objects systems and surroundingsExactlyhow entropy measures energy dispersal is mathematically simple inphase change Its just the H of the processT Further fromTables of standard state entropy the So values forsubstances at 298 K we can get a general idea of how the amount ofenergy that has been dispersed in substances differs in types ofelements and compounds Finally we can measure exactly how muchentropy increases when substances are heated ie when energy isdispersed from the surroundings to them All other areas treated ingeneral chem courses are easily describable to beginning students and I will do so but the details of their calculations can beleft to your textEntropy change shown in standard state tablesAstandard state entropy of S0 for an element or acompound is the actual change inentropy when a substance has been heated from 0 Kto 298 K However determining S0 at low temperaturesis not a simple calculation or experiment It is found either fromthe sum of actual measurements of qrevT at many increments oftemperature or from calculations based on spectroscopy The finalvalue of S0 in joulesK is related tobut not an exact figure for how muchenergy has been dispersed to the material byheating it from absolute zero where perfect crystals have anentropy of 0 to 298 KThusin our view of entropy as a measure of the amount of energydispersedT S0 is a useful rough relativenumber or index to compare substances interms of the amount of energy that has been dispersed in them from0 K For ice and liquid water the S0 at both 273 K and298 K is listed in Tables Lets consider ice at itsS0273 of 41 JK Remember that 41 joules isonly an indicator or index of the total thermal energy that wasdispersed in the mole of ice as it was warmed from 0 K Actuallyseveral thousand joules of energy were added as qrev in manysmall reversible stepsIsthat complicated Abstract and hard to understand An entropy valueof a See Answer

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