Answer to Question #312044 in Physical Chemistry for FSAFGDVCGTE3

Question

How many grams of CO2 are produced when 100 g C4H10 undergoes combustion with 200 g O2?

Use the following molar masses: C4H10=58g/mol, O2=32 g/mol and CO2=44g/mol.

Compare the moles of product formed from each reactant.

Answer 1

M(C₄H₁₀) = 58 g/mol;

M(O₂) = 32 g/mol;

M(CO₂) = 44/mol;

M(H₂O) = 18 g/mol;

m(C₄H₁₀) = 100 g;

m(O₂) = 200 g;

2C₄H₁₀ + 13O₂ = 8CO₂ + 10H₂O;

n(C₄H₁₀) = m(C₄H₁₀)/M(C₄H₁₀) = 100/58 = 1.72 mol;

n(O₂) = m(O₂)/M(O₂) = 200/32 = 6.25 mol.

Given the stoichiometric coefficients:

n(C₄H₁₀)' = n(C₄H₁₀)/2 = 0.86 mol;

n(O₂)' = n(O₂)/13 = 6.25/13 = 0.48 mol;

n(C₄H₁₀)' is higher than n(O₂)', therefore C₄H₁₀ is excess and O₂ is limited reagent.

For chemical reaction:

n(H₂O) = 10/13 * n(O₂) = 10 * 6.25/13 = 4.81 mol;

n(CO₂) = 8/13 * n(O₂) = 8 * 6.25/13 = 3.85 mol;

m(CO₂) = n(CO₂) * M(CO₂) = 3.85 * 44 = 169.4 g.

Answer: 169.4 g.