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 in the textbook, calculate the equilibrium constant for the process at room temperature.

We’re being asked to determine the equilibrium constant (K) at 25 ˚C for the given reaction:

N₂ (g) + 3H₂ (g)  →  2NH₃ (g)

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

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

We can use the following equation to solve for ΔG˚_rxn:

$\boxed{\mathbf{\Delta G}{\mathbf{°}}_{\mathbf{rxn}}\mathbf{=}\mathbf{\Delta H}{\mathbf{°}}_{\mathbf{rxn}}\mathbf{-}\mathbf{T\Delta S}{\mathbf{°}}_{\mathbf{rxn}}}$

We can get the value of the ΔH˚_rxn and ΔS˚_rxn of the reaction from the textbook or the internet. 

We have:

ΔH˚_rxn = -93 kJ/mol

ΔS˚_rxn = -198 J/K•mol

For this problem, we need to do the following steps:

Step 1: Use ΔH˚_rxn and ΔS˚_rxn to calculate for ΔG˚_rxn.

Step 2: Calculate for K.