Consider the Haber process for the synthesis of ammonia: N2(g) + 3H2(g) 2NH3(g)

Question

Consider the Haber process for the synthesis of ammonia:
N2(g) + 3H2(g) 2NH3(g)

a) At equilibrium at a certain temperature, the concentration ofNH3(g), H2(g) and N2(g) are
0.940 M, 1.60 M and 0.520 M, respectively. Calculate the value ofKc for this reaction.

b) Using the Kc you calculated in part (a), calculate KP for thisreaction at 27°C.

c) If you were to introduce into an empty ten-liter vessel 2 mol ofgaseous ammonia, 6.3 mol
of hydrogen and 2.6 mol of nitrogen, would the tendency of thereaction be to run reactants-to-products
or vice-versa? Show the calculations that provided you with thisinsight!

Explanation / Answer

             a)     N2(g) + 3H2(g) 2NH3(g)              Kc = [NH3]2 / [N2] * [H2]3                    = ( 0.94M)2 / (0.52M) * (1.6M)3                    = 0.414     b) Kp = Kc *(RT)n                 = 0.414 * ( 0.0821L.atm/mol.K* 300K)-2                 = 6.82 x 10-4    c) [NH3(g)] = 2 mol / 10 L                       = 0.2 M           [H2] =6.3mol /10L                  = 0.63 M           [N2] =2.6 mol /10 L                   =0.26 M        Since the concentrationof N2(g) and H2(g) ( reactants) are higher thereaction proceed towards the product.    c) [NH3(g)] = 2 mol / 10 L                       = 0.2 M           [H2] =6.3mol /10L                  = 0.63 M           [N2] =2.6 mol /10 L                   =0.26 M        Since the concentrationof N2(g) and H2(g) ( reactants) are higher thereaction proceed towards the product.

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.