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The change in enthalpy (ΔHorxn) for a reaction is -36.8 kJ/mol . The equilibrium constant for...

The change in enthalpy (ΔHorxn) for a reaction is -36.8 kJ/mol . The equilibrium constant for the reaction is 1.7×103 at 298 K.

What is the equilibrium constant for the reaction at 700 K ?

Express your answer using two significant figures.

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Homework Answers

Answer #1

we have relation

ln ( K2/K1) = ( dH / R) ( 1/T1 - 1/t2)

where K1 = 1.7 x 10^3 = 1700 , we need to find K2 ,

T1 = 298 K , T2 = 700K ,   dH = - 36.8 KJ/mol = -36800 J/mol, R = 8.314 J/molK

hence now ln ( K2/1700) = ( -36800J/mol /8.314J/molK) ( 1/298 - 1/700)

ln ( K2/1700) = 8.53

K2/1700 = exp ( -8.53) = 0.00019746

K2 = 1700 x 0.00019746

        = 0.336 = 0.34 ( rounded to two significant figures)

Thus equilibrium constant at 700K is 0.34

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