For each of the following pairs of substances, determine which has the larger mo

Question

For each of the following pairs of substances, determine which has the larger molar entropy at 298 K: [ (A) Cl2(g) or (B) Br2(l) ] [ (C) Fe(s) or (D) Ni(s) ] [ (E) C2H4(g) or (F) C2H6(g) ] [ (G) CCl4(g) or (H) CH4(g) ] [ (I) MgO(s) or (J) HgO(s) ] [ (K) MgCl2(aq) or (L) NaCl(aq) ]

Explanation / Answer

Higher entropy = more random/disorganized. Lower entropy = less random/disorganized. --------------------------------------… A few general rules for predicting entropy changes: 1. Gases are more random than liquids which are more random than solids. Order of increasing entropy: (s) < (l) < (g) 3C(s) + 2Fe2O3(s) -----> 4Fe(s) + 3CO2(g) 2 solids -----> 1 solid + 1 gas The formation of gas product increases entropy. 2. If the states are the same, then an increase in number of moles would mean an increase in entropy. 3C + 2Fe2O3 -----> 4Fe + 3CO2 5 moles -----> 7 moles More total moles in product increases entropy. 3. Entropy for evaporation/condensing of a liquid is much greater than that for the melting/freezing of its solid. Order of increasing entropy: melting ice

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