Question

A liquid fuel mixture contains 30.05 % hexane

(C6H14). 17.95 % heptane (C-H16),
and the rest
octane (C3H18).
the question is: what maximum mass of carbon dioxide is produced by the complete combustion of 14.0 kg of this fuel mixture?​

Answer 1

To find the maximum mass of CO2 from the combustion of a 14.0 kg liquid fuel mixture, you must calculate the mass of hexane, heptane, and octane in the mixture, then use stoichiometry with the balanced combustion equations for each hydrocarbon.

Step-by-step explanation:

The subject of this question is Chemistry, and it involves calculating the maximum mass of carbon dioxide produced from the complete combustion of a liquid fuel mixture.

First, we calculate the mass of each component in the mixture: hexane (C6H14), heptane (C7H16), and octane (C8H18). Since the liquid fuel mixture is 14.0 kg, the mass of each component would be:

• Hexane: 30.05% of 14.0 kg = 4.207 kg
• Heptane: 17.95% of 14.0 kg = 2.513 kg
• Octane: 51.00% of 14.0 kg = 7.140 kg (The rest is octane)

Next, we use the balanced equations for the combustion of each hydrocarbon to calculate the mass of CO2 produced:

1. For hexane: 2 C6H14 + 19 O2 -> 12 CO2 + 14 H2O
2. For heptane: C7H16 + 11 O2 -> 7 CO2 + 8 H2O
3. For octane: 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O

Now, apply stoichiometry to convert the mass of each hydrocarbon in the fuel to the mass of CO2 produced, taking into account the molar mass of each hydrocarbon and CO2.