Question

PROBLEMS 1) 20 points in the lab you studied the rate of a reaction by following the production of 12. A similar experiment was conducted to study the Haber process for the synthesis of ammonia. The graphs below were generated by following the production of NH3. Use the information to determine the rate law. Be sure to include the value of the rate constant. Show your work for full credit. Rate = k [N2] [H2] Ammonia Synthes | | | | | Ammonia Synthesis Nyxo) 3 Helg) - 2 MHg) | | | 000 0,04 0.035 INJ = 0.5M TH =0.5 INJ - 1.0M H -1.0M 0.03 0025 0.05 (w) CHN 20.015 0.01 0.0034 7 8 9 10 11 7 8 4 11 9 10 3 1 2 5 6 time (see) 5 6 time (sec) Ammonia Synthesis g) + 3H MT) - 24H 0.035 0.03 - OSM 0.025 0.02 0.015 0014 0.005 0 7 8 9 10 11 1 2 3 4 5 6 time (sec)

Answer 1

Haber Process is a surface reaction, hence the rate of reaction is independent of the initial concentrations of the reactants.

i.e. a = b = 0

Hence, Rate = k

Graph 1.

k = (0.004-0) M/(1-0) sec = 4*10^-3 sec^-1

Graph 2.

k = (0.008-0) M/(1-0) sec = 8*10^-3 sec^-1

Graph 3.

k = (0.004-0) M/(1-0) sec = 4*10^-3 sec^-1