L delta h 4 393509 2 241818 22267350 2511 kjmol delta

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l ) delta H= 4*-393.509+ 2*-241.818 - (2*226.73)+5*0= -2511 kj/mol delta s= 4*214 J/mol·K +2*70 J/mol·K - 2*1318.79j/mol.k-5*205 J/mol·K = -2.66658 kj/mol.k delta G = delta H- T *delta S = -2511 - 298*-2.66658= -1716.35916 kj/mol (Reference: Chang 17.17) 6. From the values of Δ H and Δ S , predict which of the following reactions would be spontaneous at 25ºC: Reaction A: Δ H = 10.5 kJ/mol, Δ S = 30 J/K ∙ mol Reaction B: Δ H = 1.8 kJ/mol, Δ S = –113 J/K ∙ mol If any of the above reactions is nonspontaneous at 25ºC, at what temperature might it become spontaneous? (16 points) Reaction A: 3 Copyright © 2014 by Thomas Edison State College. All rights reserved.
7. Calculate K P for the following reaction at 25ºC: (8 points)
Copyright © 2014 by Thomas Edison State College. All rights reserved.

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