In the important industrial process for producing ammonia (the Haber Process), the overall reaction is: N2 (g) + 3H2 (g) → 2NH3 (g) + 100.4 kJ A yield of NH3 of approximately 98% can be obtained at 200°C and 1,000 atmospheres of pressure. What is the ΔH in kJ of heat released per mole of NH3 (g) formed?

We are given the Haber Process overall reaction:

N2 (g) + 3H2 (g) = = = > 2NH3 (g) H = 100.4 kJ

Yield = 98%

T = 200 C

P = 1000 atm

We need to determine the heat released per mole of NH3 formed.

solve for the number of moles produced in the process using the ideal gas equation:

PV = nRT

1000 atm * 22.4 = n * 0.0821 L atm / mol K * (200+273) K

n = 576.82 moles * 0.98 = 565.29 moles

Therefore, the heat released per mole of NH3 is 100.4 kJ/565.29 mole NH3

ΔH = 0.1776 kJ/mole