Octane has a density of 0.692 g/ml at 20°C. Grams of O₂ required to burn 15.0 gal of C₈H₁₈ is 1.37868×10⁵g.
Octane is a hydrocarbon having eight carbon atoms and have single bonds only.
Given,
Density of octane = 0.692g/ml
Temperature = 20°C = 293K
Amount of Octane present = 15gal
Molar mass of octane = 114g
We know that,
1 gal = 3.78541L = 3785.4ml
Hence, 15 gal = 56781 ml
Now let's calculate the Mass of octane required:
Mass of octane = 0.692 x 56781
Mass of octane = 39292.45 g
According to the given equation,
C₈H₁₈ + 12.5O₂ ---------> 8CO₂ + 9H₂O
Also, 114g of octane needs-------> 400g of oxygen
39292.45g of octane needs ---------> 137868.24g of oxygen
Hence, oxygen needed to burn octane is 1.37868×10⁵g
Learn more about Octane here, brainly.com/question/21268869
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