JEE Exam > JEE Questions > 4.5 g of aluminium (atomic mass = 27 amu) is ...
Start Learning for Free
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ion in solution by the same quantity of electric charge will be
- a)22.4 L
- b)44.8 L
- c)5.6 L
- d)11.2 L
Correct answer is option 'C'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from...
From the second law of Faraday,
Or, mH = 0.5 g
2 g H2 volume at STP = 22.4 L
0.5 g H2 volume at STP 
Or, mH = 0.5 g
2 g H2 volume at STP = 22.4 L 0.5 g H2 volume at STP Free Test
FREE
| Start Free Test |
Community Answer
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from...
Given:
Mass of aluminium deposited = 4.5 g
Atomic mass of aluminium = 27 amu
To find:
Volume of hydrogen produced at STP from H ion in solution by the same quantity of electric charge
Solution:
1. Calculation of moles of aluminium deposited
Moles of aluminium deposited = Mass of aluminium deposited / Atomic mass of aluminium
= 4.5 g / 27 g/mol
= 0.1667 mol
2. Calculation of moles of electrons required for deposition of 1 mole of aluminium
Al3+ + 3e- → Al (s)
1 mole of aluminium requires 3 moles of electrons
Therefore, 0.1667 moles of aluminium will require (3 × 0.1667) moles of electrons
= 0.5 moles of electrons
3. Calculation of electric charge required for deposition of 0.5 moles of electrons
1 mole of electrons carries a charge of 96,500 coulombs (1 Faraday)
Therefore, 0.5 moles of electrons will carry a charge of (0.5 × 96,500) coulombs
= 48,250 coulombs
4. Calculation of moles of hydrogen produced from 48,250 coulombs of electric charge
1 Faraday of electric charge produces 1 mole of hydrogen gas at STP
1 Faraday = 96,500 coulombs
Therefore, 48,250 coulombs of electric charge will produce (48,250 / 96,500) moles of hydrogen gas
= 0.5 moles of hydrogen gas
5. Calculation of volume of hydrogen gas produced at STP from 0.5 moles of hydrogen gas
1 mole of any gas at STP occupies 22.4 L
Therefore, 0.5 moles of hydrogen gas will occupy (0.5 × 22.4) L at STP
= 11.2 L
Therefore, the volume of hydrogen produced at STP from H ion in solution by the same quantity of electric charge will be 11.2 L. However, the correct option given is C, which is 5.6 L. This seems to be a mistake, as the calculation above gives 11.2 L as the correct answer.
Mass of aluminium deposited = 4.5 g
Atomic mass of aluminium = 27 amu
To find:
Volume of hydrogen produced at STP from H ion in solution by the same quantity of electric charge
Solution:
1. Calculation of moles of aluminium deposited
Moles of aluminium deposited = Mass of aluminium deposited / Atomic mass of aluminium
= 4.5 g / 27 g/mol
= 0.1667 mol
2. Calculation of moles of electrons required for deposition of 1 mole of aluminium
Al3+ + 3e- → Al (s)
1 mole of aluminium requires 3 moles of electrons
Therefore, 0.1667 moles of aluminium will require (3 × 0.1667) moles of electrons
= 0.5 moles of electrons
3. Calculation of electric charge required for deposition of 0.5 moles of electrons
1 mole of electrons carries a charge of 96,500 coulombs (1 Faraday)
Therefore, 0.5 moles of electrons will carry a charge of (0.5 × 96,500) coulombs
= 48,250 coulombs
4. Calculation of moles of hydrogen produced from 48,250 coulombs of electric charge
1 Faraday of electric charge produces 1 mole of hydrogen gas at STP
1 Faraday = 96,500 coulombs
Therefore, 48,250 coulombs of electric charge will produce (48,250 / 96,500) moles of hydrogen gas
= 0.5 moles of hydrogen gas
5. Calculation of volume of hydrogen gas produced at STP from 0.5 moles of hydrogen gas
1 mole of any gas at STP occupies 22.4 L
Therefore, 0.5 moles of hydrogen gas will occupy (0.5 × 22.4) L at STP
= 11.2 L
Therefore, the volume of hydrogen produced at STP from H ion in solution by the same quantity of electric charge will be 11.2 L. However, the correct option given is C, which is 5.6 L. This seems to be a mistake, as the calculation above gives 11.2 L as the correct answer.
Attention JEE Students!
To make sure you are not studying endlessly, EduRev has designed JEE study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in JEE.
|
Explore Courses for JEE exam
|
|
Similar JEE Doubts
Top Courses for JEEView all
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer?
Question Description
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer?.
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer?.
Solutions for 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.
Here you can find the meaning of 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer?, a detailed solution for 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? has been provided alongside types of 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice 4.5 g of aluminium (atomic mass = 27 amu) is deposited at cathode from Al3+solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ion in solution by the same quantity of electric charge will bea)22.4 Lb)44.8 Lc)5.6 Ld)11.2 LCorrect answer is option 'C'. Can you explain this answer? tests, examples and also practice JEE tests.
|
|
Explore Courses for JEE exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup