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?

Question

Elle

Chemistry

1 June, 13:38

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?

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Gia Horton · 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