Repeat Example 14.4 if the burning takes place with 80% excess air.
The excess air, i.e. 80% or 0.8 will be the surplus air and will reflect as product, hence the chemical reaction will become:
C_3H_8 + 1.8 a(O_2 + 3.78 N_2) \longrightarrow bCO_2 + cH_2O + (0.8a \times d)(3.78 N_2)+ 0.8aO_2
Both side atom conservation gives:
H balance: 2 c = 8 or c = 4.
C balance: b = 3.
O balance: 2 a = z b + c or a = 5.
N balance: 2 × 3.78 a = 2d or d = 18.8
Reaction equation becomes:
C_3H_8 + (9 O_2 + 34.02 N_2) \longrightarrow 3 CO_2 + 4H_2O + 34.02 N_2 + 4 O_2
Mass fraction
for CO_2 = \frac{Mass of CO_2}{Mass of products} = \frac{Mass of CO_2}{Mass of CO_2 + Mass of H_2O + Mass of N_2 + Mass of O_2}
= \frac{\left[3 \times 44\right] }{\left[3 \times 44 + 4 \times 18 + 34.02 \times 28 + 4 \times 16\right] } = 0.108
Mass fraction
for H_2O = \frac{Mass of H_2O}{Mass of products} = \frac{Mass of H_2O}{Mass of CO_2 + Mass of H_2O + Mass of N_2 + Mass of O_2 }
= \frac{\left[4 \times 18\right] }{\left[3 \times 44 + 4 \times 18 \times 34.02 \times 28 + 4 \times 16 \right] } = 0.059