Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. the molar mass of octane is 114.33 g /mole .the molar mass of carbon dioxide is 44.0095 g/mole.
2 c8h18 +25 o2 > 16 co2 +18 h20
/\h 11018 kj

307.94g of CO₂

Explanation:

Equation of reaction

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

molarmass of C₈H₁₈ = 114.33g/mol

2 moles of C₈H₁₈ = 228.66g/mol

Molar mass of CO₂ = 44.0095g/mol

16 moles of CO₂ = 704.152g/mol

From equation of reaction,

2 moles of C₈H₁₈ reacts with 16 moles of CO₂;

228.66g of C₈H₁₈ = 704.152g of CO₂

100g of C₈H₁₈ = y moles of CO₂

y = (100 * 704.152) / 228.66

y = 307.94g of CO₂

Therefore, 100g of C₈H₁₈would yield 307.94g of CO₂.

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

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~ trueboss72