The element, s (sulfur), undergoes a phase transition from a rhombic form to a monoclinic form at 95.4°c. if δhtransition=0.38 kj mol-1, calculate δstransition under the above conditions. show all working. (ii) monoclinic sulfur is known to melt at 119°c. given δhfusion=1.23 kj mol-1, calculate, showing all working, δsfusion. (iii) given the s occurs as s8 in solid or liquid forms, convert the values of the enthalpy and entropy of fusion above to those expected for s8.

Answer:

5.6⋅10−^19  j

do you need the explaination?

Its the second one nonmetals are moldable and easily shaped 

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.