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

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