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Question

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=10.8 u, 1F=96500 C]

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,
B2H61 mol+3O23 molB2O3+3H2O2H2O(l)O2(g)+4H+(aq)+4e
Again, 27.66 g B2H6=27.6627.66=1 mol
So oxygen required is 3 mol.

Moles of O2×4=100×t96500
3×4=100×t96500
t=96500×3×43600×100 hour =965×123600=3.21 hours

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