The compound diborane was at one time considered for use as a rocket

fuel. How many grams of liquid oxygen would a rocket have to carry to

burn 14 kilograms (14,000 g) of diborane completely? *

B2H (g) + 3 O2 (g) → B2O3 (s) + 3 H2O (g)

34,690 g O₂ used.

Explanation:

Balance Equation

12B₂H + 21O₂ = > 12B₂O₃ + 6H₂O

Given 14,000g B₂H moles O₂ consumed to burn 619.47 mol B₂H

= (14,000g/22.6g/mol) = 21/12 x 619.47 mole O₂ = 1084 mole O₂

= 619.47 mol B₂H used 1084 mol O₂ x 32 g/mol = 34,690 g O₂ used.