From the reaction: B2H6 + O2 —> HBO2 + H2O What mass of H2O will be produced from burning 36.1g of B2H6

Answer 1

To solve this theoretical yield problem we have to first balance the chemical equation.

B₂H₆ + 3O₂ → 2HBO₂ + 2H₂O

We balance chemical equations because the Law of Conservation of Mass dictates that none of the reactants are lost. In this double replacement reaction some of the atoms just "change places.'

OK, so next we can figure out how much water is produced when 36.1 grams of B₂H₆ is reacted. Please remember that the coefficients to the left of the molecular formulas in the chemical equation tell us the molar ratios. Also, remember that we are going to need the molar mass of B₂H₆ and H₂O. We get those from the Periodic Table of the Elements.

36.1 g B₂H₆ x 1 mol B₂H₆ / 27.66 g B₂H₆ x 2 mol H₂O / 1 mol B₂H₆ x 18.02 g H₂O / 1 mol H₂O = 47.0 g H₂O