Question

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 296.1 g of B2H6?

Answer 1

1027.62 g

Step-by-step explanation:

For
`B_2H_6` :-

Mass of
`B_2H_6` = 296.1 g

Molar mass of
`B_2H_6` = 27.66 g/mol

The formula for the calculation of moles is shown below:

`moles = (Mass\ taken)/(Molar\ mass)`

Thus,

`Moles= (296.1\ g)/(27.66\ g/mol)`

`Moles\ of\ B_2H_6= 10.705\ mol`

From the balanced reaction:-

`B_2H_6(g) + 3 O2_((l))\rightarrow 2 HBO_2_((g))+ 2 H_2O_((l))`

1 mole of
`B_2H_6` react with 3 moles of oxygen

Thus,

10.705 mole of
`B_2H_6` react with 3*10.705 moles of oxygen

Moles of oxygen = 32.115 moles

Molar mass of oxygen gas = 31.998 g/mol

Mass = Moles * Molar mass = 32.115 * 31.998 g = 1027.62 g