RELATING IDEAS Explain why ionic crystals melt at much higher temperatures than typical covalent molecular crystals.
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Entropy Changes & Spontaneity methane from gas leak in LA reacts with O2 in atmosphere and combusts to form • water and CO2 —CH4(g) + 2O2(g)—>CO2(g) + 2H2O(l) —3 gas molecules—> 1 gas molecule + 2 liquid molecules results in decrease in entropy • ∆Ssys=∆Hsys/T • ∆Ssurr=∆Hsurr/T • ∆Suniv=∆Ssys + ∆Ssurr = ∆Ssys - (∆Hsys/T) • ex. Calculate ∆Ssys, ∆Ssurr, and ∆Suniv when 1 mole of water in ice at 0˚C melts to 22˚C. ∆H=6.01 kJ —∆Ssys=6010 J/273 K=22.0 J/K —∆Ssurr=-6010 J/295 K=-20.4 J/K —∆Suniv=22.0 J/K - 20.4 J/K=1.6 J/K • if ∆Suniv>0, the reaction is spontaneous —only ∆Suniv can determine spontaneity, not ∆Ssys (determines # microstates) • ∆Srxn=(#moles x ∆S) products - (#moles x ∆S) reactants • Gibbs free energy formula
Textbook: Modern Chemistry: Student Edition 2012
Author: Jerry L. Sarquis, Mickey Sarquis
Modern Chemistry: Student Edition 2012 was written by and is associated to the ISBN: 9780547586632. The answer to “RELATING IDEAS Explain why ionic crystals melt at much higher temperatures than typical covalent molecular crystals.” is broken down into a number of easy to follow steps, and 16 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 98 chapters, and 1789 solutions. The full step-by-step solution to problem: 10.1.19 from chapter: 10.3 was answered by , our top Chemistry solution expert on 01/04/18, 09:13PM. Since the solution to 10.1.19 from 10.3 chapter was answered, more than 337 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Modern Chemistry: Student Edition 2012, edition: 1.