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The equilibrium constant for the Haber p...

The equilibrium constant for the Haber process `3/2H_(2)+1/2N_(2)hArrNH_(3)` is 668 at 300 K and 6.04 at 400 K. What is the average of the reaction for the process in that temperature range?

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`"log"K_(2)/K_(1)=(DeltaH^(@))/(2.303R)[(T_(2)-T_(1))/(T_(1)*T_(2))]`
`"log"6.04/668=(DeltaH^(@))/(19.09)[(400-300)/(300xx400)]`
`log9.042xx10^(-3)=(DeltaH^(@))/19.09(100/120000)`
`-2.044=(DeltaH^(@))/22908`
`thereforeDeltaH^(@)=-2.044xx22908`
= -46818 J/mol
= -47 kJ/mol
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