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Heat of combustion of diborane is 1976 kJ/mole. Which of the following is correct if 19.76 kJ of energy is released during reaction

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0.3 moles of oxygen is consumed

0.54 gm of water is formed

0.1 mole of B₂O₃ is formed

0.05 mole of diborane is burnt

answer is B.

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Detailed Solution

B₂H₆ + 3O₂ $\to$ B₂O₃ + 3H₂O; $∆ H_{c}$ = - 1976 kJ/mole

mass of water formed = $\frac{3 \times 18 \times 19.76}{1976}$ = 0.54 gm

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