A mixture of hydrocarbons contains 36.6 % heptane, C7H16, 13.4 % nonane, C9H20, and 50.0 % octane, C8H18. The mixture is combusted in an excess of oxygen. What mass of CO2 is generated from the combustion of 11.0 kg of the mixture?

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pucesnail37Lv1

24 Feb 2020

A mixture of hydrocarbons contains 36.6 % heptane, C₇H₁₆, 13.4 % nonane, C₉H₂₀, and 50.0 % octane, C₈H₁₈. The mixture is combusted in an excess of oxygen. What mass of CO₂ is generated from the combustion of 11.0 kg of the mixture?

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The octane rating of gasoline is a relationship of the burningefficiency of the given gasoline mixture to the burning efficiencyof octane (C8H18). (Figure1) Like most hydrocarbons, octane reacts with oxygen gas toproduce carbon dioxide and water. The unbalanced equation for thisreaction is C8H18(g) + O2(g) ? CO2(g) + H2O(g).

Balanced chemical equation is 2C8H18(g) + 25O2(g) ?16CO2(g) + 18H2O(g).

A)-How many moles of water are produced in this reaction?

B)- After the reaction, how much octane is left?

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orangeoyster501

A technician for the Ethanol-in-Octane fuel company was testing amixture of ethanol and octane as a synthetic fuel. Combustion of asample of this mixture of ethanol and octane (in the presence ofexcess oxygen) produced 208.09 g of water and 439.34 g of carbondioxide. Determine the mass percent ethanol in the sample used forthe analysis. (The technician forgot to record the mass of thesample used in the analysis. Because he knows the mass of waterproduced and the mass of CO2 produced he does not need the mass ofthe sample.) The balanced equations for the combustion of ethanoland octane are shown below.

ethanol: 1 C2H5OH + 3 O2 -> 2 CO2 + 3 H2O
octane: 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O

C2H5OH molar mass 46.07; C8H18 molar mass 114.22
H2O molar mass 18.02; CO2 molar mass 44.01

I guess I need to use system of equation to solve thisproblem, but I have no clue how to set up the equation.

P.S The answer is mass percent of ethanol = 13.1%, but I don'tknow why. Please show me the steps, thanks!