Question

The compound diborane (b2h6) was at one time considered for use as a rocket fuel. its combustion reaction is b2h6(g) + 3 o2(â) â 2 hbo2(g) + 2 h2o(â) 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 106.3 g of b2h6?

Answer 1

The atomic mas of Oxygen gas is 32 g/mol
The molar mass of B2H6 IS 27.66 g/mol
Therefore, a mass of 106.3 g of B2H6 will contain;
     106.3/27.66 =  3.843 moles
The mole ratio of B2H6 : O2 is 1: 3
Therefore, moles of oxygen will be 3.843 ×3/1 = 11.529 moles
Therefore, the mass of liquid oxygen needed would be;
11.529 × 32
= 368.94 g