Problem 2: What is the entropy of transition between orthorhombic sulfur 𝛼 and monoclinic sulfur 𝛽 if the transition enthalpy is 402 𝐽𝑚−1 at the transition temperature 369 K
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Two allotropes ( $A$ and $B$ ) of sulfur interconvert at $369 \mathrm{K}$ and 1 atm pressure:$$\mathrm{S}_{\mathrm{s}}(s, \mathrm{A}) \rightarrow \mathrm{S}_{\mathrm{g}}(s, \mathrm{B})$$.The enthalpy change in this transition is $297 \mathrm{J} / \mathrm{mol}$. What is the entropy change?
Nicole S.
You are contemplating rhombic sulfur and monoclinic sulfur. The density of rhombic sulfur is 2.070 g cm-3 with a standard molar entropy of 31.80 J K-1 mol-1. The density of monoclinic sulfur is 1.957 g cm-3 with a standard molar entropy of 32.60 J K-1 mol-1. The standard Gibbs energy of formation of rhombic sulfur is zero and that of monoclinic sulfur is 0.33 kJ mol-1 at 25 C. Calculate what temperature the transition occurs at with 1 bar pressure. (3 sig figs, units of K)
Yash K.
At the transition temperature of 95.4°C, the enthalpy of transition from rhombic to monoclinic sulfur is 0.38 kJ mol⁻¹. a. Calculate the entropy of transition under these conditions. b. At its melting point, 119°C, the enthalpy of fusion of monoclinic sulfur is 1.23 kJ mol⁻¹. Calculate the entropy of fusion. c. The values given in parts (a) and (b) are for 1 mol of sulfur; however, in crystalline and liquid sulfur, the molecule is present as S₈. Convert the values of the enthalpy and entropy of fusion in parts (a) and (b) to those appropriate for S₈.
Adi S.
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