the balanced reaction equation for the combustion of butane is as follows; C₄H₁₀ + 13/2O₂ ---> 4CO₂ + 5H₂O the limiting reactant in this reaction is C₄H₁₀ This means that all the butane moles are consumed and amount of product formed depends on the amount of C₄H₁₀ used up. stoichiometry of C₄H₁₀ to H₂O is 1:5 mass of butane used - 6.97 g number of moles - 6.97 g / 58 g/mol = 0.12 mol then the number of water moles produced - 0.12 mol x 5 = 0.6 mol Therefore mass of water produced - 0.6 mol x 18 g/mol = 10.8 g
