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.

🤓 Based on our data, we think this question is relevant for Professor Collins' class at OSU.

FREE Expert Solution

N2(g) + 3 H2(g)  →  2 NH3(g)


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


ΔG°rxn=-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:

View Complete Written Solution
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.