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.

FREE Expert Solution

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:


ΔG°rxn=-RTlnK


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


ΔG°rxn=ΔH°rxn-TΔS°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.


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