Determine how many grams of CO2 are produced by burning 2.43g of C4H10

Answer 1

First, we must write a correctly balanced equation for the reaction taking place.

2 C₄H₁₀ + 13 O₂ ==> 8 CO₂ + 10 H₂O ... balanced equatin

Next, we find the MOLES of C₄H₁₀, then moles CO₂ produced, and finally grams CO₂ produced.

molar mass C₄H₁₀ = 58 g / mol

molar mass CO₂ = 44 g / mol

2.43 g C₄H₁₀ x 1 mol / 58 g = 0.0419 mols C₄H₁₀

0.0419 mol C₄H₁₀ x 8 mol CO₂ / 2 mol C₄H₁₀ = 0.168 mol CO₂

0.168 mol CO₂ x 44 g CO₂ / mol = 7.37 g CO₂ produced