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n-Octane (C8H18) is burned with 60 percent excess air with 15 percent of the carbon in the fuel forming carbon monoxide. Calculate the mole fractions of the products and the dew-point temperature of the water vapor in the products when the products are at 1.3 atm pressure. Use data from the tables.The mole fraction of CO2 is .0678the mole fraction of CO is .012the mole fraction of H2O is .0897the mole fraction of O2 is .0808and the mole fraction of N2 is .7498The dew-point temperature of the water vapor is _____°C.

Respuesta :

Answer:

The answer is "[tex]49.23^{\circ}[/tex]"

Explanation:

The mole fraction of water vactor [tex](x_w)[/tex]

[tex]\to x_w= 0.0897[/tex]

Total pressure of product [tex]= \Delta P = 1.3 atm[/tex]

[tex]=P =1.317 \ bar[/tex]

partial pressue  of the water vapour (P_w)

[tex]P_w = p.X_w \\\\[/tex]

     [tex]=1.317 \times 0.0897\\\\= 0.118 \ bar[/tex]

stram table   at 0.118 bar saturation tempreature  [tex]T_{sat} =49.23^{\circ}[/tex]

Dew to point temprature of water vapour is [tex]49.23^{\circ}[/tex]

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