Question

The reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3 H2(g) + 2 NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 2.98 x 10-5 mol L-15-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed? N2 is consumed at the rate of mol L-15-1 H2 is consumed at the rate of mol L-15-1

Answer 1

Balanced chemical equation: N2(g)+ 3H2(g) + 2NH,(g) According rate law: d[N]_id[H]_1d[NH] dt 3 dt 2 dt d[NH) – 298x10-mole Los dt q[N.] apart = (2.98x10- moke -1.9103 mola Los = 1.49x10-5 mole Los |id[H]_1d[NH ] 3 dt 2 dt (14,1- (2.98-105 m.hk) = 4.47x10-5 mole Los