Question

A mixture of perfect gases consists of 3 kg of carbon monoxide and 1.5 kg of nitrogen at a pressure of 0.1 MPa and a temperature of 298.15 K. Using Table 5-1, find (a) the effective molecular mass of the mixture, (b) its gas constant, (c) specific heat ratio, (d) partial pressures, and (e) density.

Table 5-1 comes from Rocket Propultion Elements volume 8.

Answer 1

without using the table.. i am using the values we generally use.

moles of CO = 3000/28 = 107.14

moles of N₂ = 1500/28 = 53.57

a) as both gases have molar mass of 28 g so effective molar mass is also 28g

b) gas constant = 8.314 J/Kmole

c) specific heat of CO/specific heat of N₂ = 1.04(J/gK)/1.04(J/gK) = 1

d) partial pressure of CO = 0.1 x 3/4.5 = 0.066666 MPa

partial pressure of N₂ = 0.1 x 1.5/4.5 = 0.03333 MPa

density = 100000 x 0.028/8.3.14 x 298.15 = 1.129 kg/m³