Question

The compound diborane (B₂H6) was at one

time considered for use as a rocket fuel. Its
combustion reaction is
B2H6(g) + 3 O2(l) → 2 HBO2(g) + 2 H₂O(l)
The fact that HBO2, a reactive compound,
was produced rather than the relatively inert
B₂O3 was a factor in the discontinuation of
the investigation of the diborane as a fuel.
What mass of liquid oxygen (LOX) would be
needed to burn 190.3 g of B₂H6?
Answer in units of g. Answer in units of g.

Answer 1

1583.76 g O2

Step-by-step explanation:

For every one molecule of B2H6 that reacts, 3 molecules of O2 are needed. To determine the mass of liquid oxygen (LOX) needed to burn 190.3 g of B2H6, use the balanced equation as a conversion factor.

1 mole of B2H6 = 28.02 g

1 mole of O2 = 32 g

Using the balanced equation above, you know that for every 1 mole of B2H6, 3 moles of O2 are needed.

Therefore, the mass of O2 needed for 190.3 g of B2H6 is:

190.3 g B2H6 * (3 moles O2 / 1 mole B2H6) * (32 g O2 / 1 mole O2) = 1583.76 g O2