Consider the following chain-reaction mechanism for the high-temperature formation of nitric oxide, i.e., the Zeldovich mechanism: O+N2k1fNO+NReaction1N+O2k2yNO+OReaction2 A. Write out expressions 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. (Answer: d[NO]/dt=2k1f[Oeq[N2]eq ) C. Write out the expression for the steady-state N-atom concentration used in part B. D. For the conditions given below and using the assumptions of part B, how long does it take to form 50ppm (mole fraction 106 ) of NO? TMW0,eqO,egN2,efk1f=2100K,=0.167kg/m3,=28.778kg/kmol,=7.6105(molefraction),=3.025103(molefraction),=0.726(molefraction),=1.821014exp[38,370/T(K)]withunitsofcm3/gmols. E. Calculate the value of the reverse reaction rate coefficient for the first reaction, i.e., O+N2NO+N, for a temperature of 2100K. F. For your computations in part D, how good is the assumption that reverse reactions are negligible? Be quantitative. G. For the conditions of part D, determine numerical values for [N] and N. (Note: k2f=1.81010Texp(4680/T) with units of cm3/gmols.)