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The change in enthalpy (ΔHorxn) for a reaction is -24.4 kJ/mol . The equilibrium constant for...

The change in enthalpy (ΔHorxn) for a reaction is -24.4 kJ/mol . The equilibrium constant for the reaction is 1.5×103 at 298 K.What is the equilibrium constant for the reaction at 675 K?

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Answer #1

log(K2/K1) =- H/2.303*R [1/T1-1/T2]

log(1.5*10^3/K1) = -24400/2.303*8.314 [1/298 -1/675]

log(1.5*10^3/K1) =-1274.34 (0.00335 -0.00148)

log(1.5*10^3/K1)   = -2.3830

(1.5*10^3/K1)        = 10^-2.3830

(1.5*10^3/K1)         = 0.00414

K1                         = 1.5*10^3/0.00414    = 3.6*10^5 >>>>>answer

  

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