The Haber Bosch Process is a critically important chemical reaction run on an industrial scale. The reaction is shown below: 3 H₂+N2 =2 NH3 a) Using the thermodynamic tables in your textbook determine the ΔH, ΔS, and ΔG of this reaction at 298 K and 1 bar. b) Calculate the equilibrium constant at 298 K. What conclusions can you draw about this reaction at low pressure and temperatures? c) This reaction is typically run at elevated temperatures and pressure to improve reaction yield. What impact would increased pressure have on ΔG? What about increased temperature? Justify your answers! d) The actual equilibrium constant at 1000K is K = 5.85 x 10-4. Determine the value of ΔG.

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a To determine the H S and G of the Haber Bosch Process at 298 K and 1 bar we need to refer to the t... View the full answer