Consider the following chain-reaction mechanism for the high- temperature formation of nitric oxide (the Zeldovich mechanism): k 1f k N+O NO+O 2 O+N NO+N 1 2 2f 2 a. Write out expression for d[NO]/dt and d[N]/dt. b. Assuming N atoms exist in steady-state and that the concentrations of O, O2, and N2 are at their equilibrium values for a specified temperature and composition, simplify your expression obtained above for d[NO]/dt for the case of negligible reverse reactions. c. Write out the expression for the steady-state N-atom concentration used in part (b). d. For the following conditions and using the assumptions of part (b), how long does it take to form 50 PPM of NO? T=2,100K =0.167 kg/m3 MW=28.778 O,eq=7.6x10-5 O2,eq=3.025x10-3 N2,eq=0.726 k1f=1.82x1014exp[-38,370/T] with units of cm3/gmol s e. Calculate the value of the reverse reaction rate coefficient for the first reaction, for a temperature of 2,100 K f. For the calculations of part (d), how good is the assumption that the reverse reactions are negligible (give a quantitative answer). g. For the conditions of part (d), determine numerical values for [N] and N using k2f=1.8x1010Texp(-4,680/T) with units of cm3/gmol s)