How long (approximate) should water be electrolysed by passing through 100 amperes current so that the oxygen released can completely burn 27.66 g of diborane?
[Atomic weight of B=10.8u, 1F=96500C]
A
3.2 hours
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B
1.6 hours
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C
6.4 hours
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D
0.8 hour
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Solution
The correct option is A 3.2 hours The corresponding reactions are, B2H61mol+3O23mol→B2O3+3H2O2H2O(l)→O2(g)+4H+(aq)+4e−
Again, 27.66gB2H6=27.6627.66=1mol
So oxygen required is 3 mol.
∴ Moles of O2×4=100×t96500 ⇒3×4=100×t96500 ⇒t=96500×3×43600×100hour=965×123600=3.21hours