A fuel is prepared by mixing 4 moles of argon (Ar, inert) with 12 moles of ethane (C2H6) and 6 moles of propane (C3H8) and undergoes complete combustion in air according to the following reactions: C2H6 + 7/2 O2 reacts to form 2 CO2 + 3 H2O C3H8 + 5 O2 reacts to form 3 CO2 + 4 H2O Air may be considered as 21 mol% oxygen (O2) and 79 mol% Nitrogen (N2). The average molecular mass of a mixture can be calculated as Maverage = Σ xi Mi where xi and Mi are mole fraction and molecular mass of component i. Atomic masses: C = 12; O = 16; H = 1; N = 14; Ar = 40. Calculate: a. the theoretical air required to burn the fuel (in kg air per kg fuel) b. the mole fraction of CO2 on a wet basis in the flue gas if the fuel is burned with 30% excess air, assuming complete combustion
A fuel is prepared by mixing 4 moles of argon (Ar, inert) with 12 moles of ethane (C2H6) and 6 moles of propane (C3H8) and undergoes complete combustion in air according to the following reactions: C2H6 + 7/2 O2 reacts to form 2 CO2 + 3 H2O C3H8 + 5 O2 reacts to form 3 CO2 + 4 H2O Air may be considered as 21 mol% oxygen (O2) and 79 mol% Nitrogen (N2). The average molecular mass of a mixture can be calculated as Maverage = Σ xi Mi where xi and Mi are mole fraction and molecular mass of component i. Atomic masses: C = 12; O = 16; H = 1; N = 14; Ar = 40. Calculate: a. the theoretical air required to burn the fuel (in kg air per kg fuel) b. the mole fraction of CO2 on a wet basis in the flue gas if the fuel is burned with 30% excess air, assuming complete combustion
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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A fuel is prepared by mixing 4 moles of argon (Ar, inert) with 12 moles of ethane (C2H6) and 6
moles of propane (C3H8) and undergoes complete combustion in air according to the following
reactions:
C2H6 + 7/2 O2 reacts to form 2 CO2 + 3 H2O
C3H8 + 5 O2 reacts to form 3 CO2 + 4 H2O
Air may be considered as 21 mol% oxygen (O2) and 79 mol% Nitrogen (N2).
The average molecular mass of a mixture can be calculated as Maverage = Σ xi Mi where xi and Mi are mole
fraction and molecular mass of component i. Atomic masses: C = 12; O = 16; H = 1; N = 14; Ar = 40.
Calculate:
a. the theoretical air required to burn the fuel (in kg air per kg fuel)
b. the mole fraction of CO2 on a wet basis in the flue gas if the fuel is burned with 30% excess air,
assuming complete combustion
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