Question

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?
50.2 kJ
-50.2 kJ
100.4 kJ
-100.4 kJ

Answer 1

Answer:

- 50.2 kJ

Explanation:

• From the data given, the heat released per 2.0 moles of NH₃ is - 100.4 kJ.

• The negative sign means that the reaction is exothermic and the energy is released.

• So, the ΔH in kJ of heat released per mole of NH₃ formed is (100.4 kJ/2) = - 50.2 kJ.