# Problem: The Haber process is the principal industrial route for converting nitrogen into ammonia:N2 (g) + 3H2 (g)  →  2NH3 (g).Using the thermodynamic data in Appendix C, calculate the equilibrium constant for the process at room temperature.Calculate the standard emf of the Haber process at room temperature.

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###### FREE Expert Solution

N2(g) + 3 H2(g)  →  2 NH3(g)

Recall that ΔG˚rxn and K are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

We’re given the ΔH˚f and S˚ of each reactant and product:

 Substance ΔH˚f (kJ/mol) S˚ (J/mol • K) N2(g) 0 191.61 H2(g) 0 130.68 NH3(g) – 46.11 192.45

Step 1: We can use the following equation to solve for ΔH˚rxn:

###### Problem Details

The Haber process is the principal industrial route for converting nitrogen into ammonia:
N2 (g) + 3H2 (g)  →  2NH3 (g).

Using the thermodynamic data in Appendix C, calculate the equilibrium constant for the process at room temperature.

Calculate the standard emf of the Haber process at room temperature.