please help within five minutes

Question Description

sulfur undergoes a phase change from the rhombic crystal structure to the monoclinic form at 95.3 °C. 

Assuming that ΔH for this phase change is 0.202 kJ/mol, calculate ΔS for this phase change.

Final Answer

We need to use the Gibbs Free Energy equation....

G = H - TS     (I've omitted the deltas, but assume they are there)

H = 0.202 KJ/mol = 202 J/mol

T = 273 + 95.3 = 368.3 K

Assume, G = 0 KJ/mol

So essentially, H = TS.  Solving for S...

S = H/T = 202J/mol / 368.3 K 

= 0.548 J/K/mol

Steve_R944 (190)
Cornell University

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