Solution Found!
The analysis on a mass basis of an ideal gas mixture at
Chapter 12, Problem 12.1(choose chapter or problem)
The analysis on a mass basis of an ideal gas mixture at \(50^{\circ} \mathrm{F}\), \(25 \mathrm{lbf} / \mathrm{in}^{2}\) is 60% \(\mathrm{CO}_{2}\), 25% \(\mathrm{SO}_{2}), and 15% \(\mathrm{N}_{2}\). Determine
(a) the analysis in terms of mole fractions.
(b) the apparent molecular weight of the mixture.
(c) the partial pressure of each component, in \(\mathrm{lbf} / \mathrm{in}^{2}\)
(d) the volume occupied by 20 lb of the mixture, in \(\mathrm{ft}^{3}\).
Questions & Answers
QUESTION:
The analysis on a mass basis of an ideal gas mixture at \(50^{\circ} \mathrm{F}\), \(25 \mathrm{lbf} / \mathrm{in}^{2}\) is 60% \(\mathrm{CO}_{2}\), 25% \(\mathrm{SO}_{2}), and 15% \(\mathrm{N}_{2}\). Determine
(a) the analysis in terms of mole fractions.
(b) the apparent molecular weight of the mixture.
(c) the partial pressure of each component, in \(\mathrm{lbf} / \mathrm{in}^{2}\)
(d) the volume occupied by 20 lb of the mixture, in \(\mathrm{ft}^{3}\).
ANSWER:Step 1 of 4
a) To calculate the mole fractions of the given gas mixture we will use the given mass analysis and . For the calculation we will assume the mass of the mixture is and we will also need the molar masses for each gas which we will take from the molar mass tables.
The mixture number of moles is then:
The mole fractions are then: