Determine the entropy change when 1.80 mol of HBr(g) condenses at atmospheric pressure?
I got that DeltaS fus = 12.922J/(k*mol)
Delta S Vapour = 93.475J/(K*mol)
the only thing I don't get is the entropy change when 1.80 mol of HBr(g) condenses at atmospheric pressure. How do I do it?! I got an answer of -23.2596J/K because I multiplied the DeltaS fuion by the molar ratio and flipped the sign (-12.922*1.80) and got the wrong answer :-( The prompt says incorrect and "The value of ΔSvap above is for 1.00 mol of HBr. You need to scale that value up for 1.80 mol of HBr. Also, consider the sign of your answer. Does condensing result in an increase or decrease in entropy?" So I give up. anyone please help me get the value of DeltaS for HBr!
Extra Info;
Melting Point = -86.96 cel,
Delta h fusion = 2.406
boiling point = -67.0 cel,
delta h vapour = 19.27 kj/mol
(this is all the info they gave for HBr in the question) thank you in advance!
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