How long (approximate) should water be electrolysed by passing...

${B}_{2}{H}_{6} + 3{O}_{2} \to {B}_{2}{O}_{3} + 3{H}_{2}O$
According to balanced equation
27.66 g ${B}_{2}{H}_{6}$ i.e. 1 mole ${B}_{2}{H}_{6}$ requires 3 mole of ${O}_{2}$ . Now this oxygen is produced by electrolysis of water as follows
$2{H}_{2}O\overset{4F}{\to}2{H}_{2} + {O}_{2}$
As 1 mole ${O}_{2}$ is produced by 4 F charge
So 3 mole ${O}_{2}$ will be produced by 12 F charge
So now on applying
Q = It
$\text{12} \times \text{965}00C = 100 \times t ( s )$
$t = \dfrac{12 \times 96500}{100 \times 3600}$ hours
$t = 3.2$ hours