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 per mole of NH3(g) formed?

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 per mole of NH3(g) formed?

aaronq · Answer

$\nu_i*\Delta H^i_f=2*\Delta H^{NH_3}_f=100.4~ kJ$


$\Delta H^{NH_3}_f=\dfrac{100.4~kJ}{2}$

aaronq · Answer

I used the simplification in writing the formula with the fact that $\Delta H_f=0$ for both, $N_2$ and $H_2$.