Reference no: EM131207117
Problem 1
For the global reaction v'FCmHn + v'O_2 O2 = v''CO_2 CO2 + v''H_2O H2O calculate the stoichiometric mixture fraction and the adiabatic flame temperature for the following fuels, if both fuel and oxygen are pure (no N2) and in the unburned at T = 298.16K: CH4, C2H4, and C3H8. Use cp = 1.2kEka . Document all your solution steps.
For bonus points, use NASA polynomials and solve numerically if the oxidizer stream contains 50% mass-fraction of N2.
Problem 2
Consider the global reaction
H2 + 1/2O2 = H2O (1)
in a stoichiometric hydrogen/oxygen system. Document all your solution steps.
a) Calculate the unburned mass fractions of oxygen and hydrogen, YO_2,u and YH_2O.
b) Calculate the element mass fractions of H and 0 in the system.
c) For T = 2000K, T = 3000K, and T = 4000K at p = lbar and p = 10bar, calculate the chemical equilibrium compositions of H2, O2, and H2O. Compare these values to those for complete combustion. (Hint: you can find a closed solution for this by expressing, for example, YH2O as a function of the element mass fractions, the equilibrium constant, and pressure.)
d) Discuss the observed trends of c) for increasing temperate and increasing pressure.
Problem 3
Consider an adiabatic two feed system at p = lbar, where the fuel stream consists of pure H2O at T = 298.16K and the oxidizer stream is pure O2 at T = 298.16K. The global reaction is
H2 + 1/2O2 = H2O (2)
Calculate and plot as a function of mixture fraction the temperature and the mass fractions of H2, O2, and H2O in the burnt for
a) complete combustion,
b) chemical equilibrium.
Document all your solution steps. Upload any code you used to solve this problem to the Homework Blackboard link. No credit will be given if the code is not uploaded.
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