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A reaction has an equilibrium constant of 8.2×103 at 298 K. At 751 K , the...

A reaction has an equilibrium constant of 8.2×103 at 298 K. At 751 K , the equilibrium constant is 0.90. Find ΔHorxn for the reaction.

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Answer #1

K1 = 8.2*103     T1 = 298K

K2 = 0.9             T2 = 751K

logK2/K1   = H/2.303R [1/T1-1/T2]

log0.9/8200 = H/2.303*8.314 [1/298 -1/751]

-3.9595        = H/19.147 (0.00335-0.00133)

H           = -3.9595*19.147/0.00202   = -37530.96J

   H      = -37.530KJ

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