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)

1) 0.8 hours

2) 3.2 hours

3) 1.6 hours

4) 6.4 hours

Answer: (2)

B2H6 +3O2 -> B2O3 +3H2O

27.66 of B2H6 = 1 mole of B2H6 which requires three moles of oxygen (O2) for complete burning

6H2O -> 6H2 +3O2 (On electrolysis)

Number of faradays = 12 = amount of charge

12×96500 = i×t

12×96500 = 100×t

t = 12×96500/100 sec

t = 12×96500/(100×3600) hour

t = 3.2 hours

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