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Write the combustion equation with no hydrogen in the products and then use the water-gas reaction to estimate the amount of hydrogen present.
It is heated in a constant-pressure process, so the mole fraction of atomic hydrogen, H, is 10%. Find the final temperature and the heat transfer needed.
How should the adiabatic flame temperature be found if the equilibrium reaction 2H2 + O2 ? 2H2O is considered? Disregard all other possible reactions.
Catalytic gas generators are frequently used to decompose a liquid. Calculate the mole fractions of the species in the equilibrium mixture.
One approach to using hydrocarbon fuels in a fuel cell is to reform. Determine the equilibrium constant for this reaction at a temperature of 800 K.
Butane is burned with 200% theoretical air, and the products of combustion, an equilibrium mixture. Determine the equilibrium composition at this state.
Find the equilibrium composition at this state, assuming that only N2, O2, NO, O, and Ar are present.
Assume we only have H2O, O2, OH, and H2 as gases with the two simple water dissociation reactions active. Find the equilibrium composition.
Calculate the equilibrium composition of the mixture leaving the converter. Would it be more desirable to operate the converter at ambient pressure?
At 10 000 K the ionization reaction for argon as Ar ? Ar+ + e- has a constant. What should the pressure be for a mole concentration of argon ions (Ar+) of 10%?
Assume air is at 3000 K, 1 MPa. Find the time constant for NO formation. Repeat for 2000 K, 800 kPa.
For a mixture of O2 and O the pressure is increased at constant T; what happens to the composition?
For nearly all the dissociations and ionization reactions, what happens to the composition when the pressure is raised?
What is the equilibrium mole fraction of NO? Find the enthalpy difference in the gases due to the formation of the NO.
Pure oxygen is heated from 25oC, 100 kPa, to 3200 K in a constant-volume container. Find the final pressure, composition, and heat transfer.
Assume the dissociation of CO2 is the only equilibrium process to be considered. Find the exit equilibrium composition and the heat transfer rate.
Assuming that only these substances are present in the exiting chemical equilibrium mixture, determine the composition of that mixture.
Compute the temperature of the products exiting the chamber. Assume that only H2O, H2, and N2 are present.
What is the temperature of the products exiting the combustor? Find the adiabatic flame temperature, assuming complete combustion.
Calculate x if half the water in the products is condensed. Calculate the absolute entropy of the products at the exit conditions.
The mixture is lean, so the adiabatic flame temperature is 3200 R. Find the entropy generation per lbmol fuel, neglecting all the partial pressure corrections.
How much mass of water is condensed per pound-mass of fuel? Repeat the problem, assuming that the air used in the combustion has a relative humidity of 90%.
Find the efficiency of the engine expressed as (work/lower heating value) and the second-law efficiency.
Find the mixture temperature before combustion and also the work, assuming an adiabatic turbine.
Write a program to study the effect of the percentage of theoretical air on the adiabatic flame temperature for a (variable) hydrocarbon fuel.