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Faradays law of electrolysis

How long (approximate) should water be electrolysed by passing

Question

Medium

Solving time: 3 mins

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 $B = 10.8 μ$ )

6.4 hours

0.8

hours

3.2

hours

1.6

hours

Views: 5,430 students

Updated on: May 26, 2023

Book:

Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

Exam:

JEE Mains 2018

Found 2 tutors discussing this question

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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 μ

)

11 mins ago

Discuss this question LIVE

11 mins ago

Text solutionVerified

Given that,

i = 100 amp

. also,

27.66 g

of diborane

(B_{2} H_{6})

Molecular mass of

B_{2} H_{6} = 10.8 \times 2 + 6 = 27.6

Number of moles of

B_{2} H_{6}

27.66 g

= \frac{Given mass}{Molar mass} = \frac{27.66}{27.6} \approx 1

Now consider the equation

B_{2} H_{6} + 3 O_{2} ⟶ B_{2} O_{3} + 3 H_{2} O

From the equation we can interpret that 3 moles of oxygen is required to burn 1 mole (i.e.

27.6 g

)

B_{2} H_{6}

completely. Also consider the electrolysis reaction of water i.e.

H_{2} O ⇌ 2 H^{+} + O^{--}

2 H^{+} Cathode ⟶ + 2 e^{-} 2 H ⟶ H_{2} ↑

O^{-} ⟶ - 2 e^{-} Anode O atoms ⟶ 2 such O_{2} ↑

From the above equation it can be easily interpreted that in electrolysis of water for the production of 1 mole of oxygen from 1 mole of

H_{2} O

at anode 4 moles electrons are required. Likewise for the production of 3 moles of

O_{2}

12 (3 \times 4)

moles of electrons will be needed. So, the total amount of charge required to produce 3 moles of oxygen will be

12 \times F

12 \times 96500

We know

Q = it

So,

12 \times 96500 = 100 \times t

in seconds or

\frac{12 \times 96500}{100 \times 3600} = t

in hours

= 3.2

hours

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Question Text	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 $B = 10.8 μ$ )
Updated On	May 26, 2023
Topic	Electrochemistry
Subject	Chemistry
Class	Class 12
Answer Type	Text solution:1 Video solution: 3
Upvotes	409
Avg. Video Duration	7 min

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 $B = 10.8 μ$ )

Text solutionVerified

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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=10.8μ )

Text solutionVerified

Filo tutor solutions (3)

Questions from JEE Mains 2018 - PYQs

Practice questions from Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

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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 $B = 10.8 μ$ )