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Question

How long (approximate) should water be electrolyzed by passing through 100 amperes current so that the oxygen released can completely burn 27.66g of diborane ? (Atomic weight of B=10.8u)?


A

0.8 hours

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B

3.2 hours

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C

1.6 hours

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D

6.4 hours

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Solution

The correct option is B

3.2 hours


Explanation for the correct options:

B) 3.2 hours

Step 1: i=100 amperes, 27.66g of diborane

Step 2: Faraday's Law =mass of the substance deposited during electrolysis × quantity of electricity passing

Step 3: Reaction involved B2H6+3O2B2O3+3H2O

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

6H2O6H2+3O2 (On electrolysis)

On electrolysis of water, 2H2OO2+4H++4e

1 mole of O2 is produced by 4F charge.

Then, 3 mole of O2 will require 12F charge.

Now applying, q=it

12×96500=i×t12×96500=100×tt=12×96500/100sect=12×96500/(100×3600)hr.t=3.2

Therefore, time taken for water to be electrolyzed is 3.2 hours

Explanation for the incorrect option:

(A) The above detailed explanation clearly explains option A is incorrect.

(C) The above detailed explanation clearly explains option C is incorrect.

(D) The above detailed explanation clearly explains option D is incorrect.

Hence, option B is correct.


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