NEET Exam > NEET Questions > Some quantity of electricity is used to liber...
Start Learning for Free
Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g?
Most Upvoted Answer
Some quantity of electricity is used to liberate iodine at anode and a...
Community Answer
Some quantity of electricity is used to liberate iodine at anode and a...
Calculation of Equivalent Mass of Metal:
Given Data:
- Mass of metal deposited = 0.617g
- Volume of 0.124 molar Na2S2O3 solution used to reduce iodine = 46.3ml
Step 1: Calculate the moles of iodine reduced
- Moles of iodine = Molarity * Volume (in liters)
- Moles of iodine = 0.124 mol/L * 0.0463 L
- Moles of iodine = 0.00574 mol
Step 2: Calculate the moles of metal deposited
- Moles of metal = Moles of iodine (since they are in 1:1 ratio)
- Moles of metal = 0.00574 mol
Step 3: Calculate the molar mass of the metal
- Molar mass of metal = Mass of metal deposited / Moles of metal
- Molar mass of metal = 0.617g / 0.00574 mol
- Molar mass of metal ≈ 107.6 g/mol
Step 4: Calculate the equivalent mass of metal
- Equivalent mass = Molar mass / Valency
- Since the metal was deposited at the cathode, its valency is 1
- Equivalent mass = 107.6 g/mol / 1
- Equivalent mass ≈ 107g
Therefore, the equivalent mass of the metal deposited is approximately 107g. Hence, the correct answer is option B.
Given Data:
- Mass of metal deposited = 0.617g
- Volume of 0.124 molar Na2S2O3 solution used to reduce iodine = 46.3ml
Step 1: Calculate the moles of iodine reduced
- Moles of iodine = Molarity * Volume (in liters)
- Moles of iodine = 0.124 mol/L * 0.0463 L
- Moles of iodine = 0.00574 mol
Step 2: Calculate the moles of metal deposited
- Moles of metal = Moles of iodine (since they are in 1:1 ratio)
- Moles of metal = 0.00574 mol
Step 3: Calculate the molar mass of the metal
- Molar mass of metal = Mass of metal deposited / Moles of metal
- Molar mass of metal = 0.617g / 0.00574 mol
- Molar mass of metal ≈ 107.6 g/mol
Step 4: Calculate the equivalent mass of metal
- Equivalent mass = Molar mass / Valency
- Since the metal was deposited at the cathode, its valency is 1
- Equivalent mass = 107.6 g/mol / 1
- Equivalent mass ≈ 107g
Therefore, the equivalent mass of the metal deposited is approximately 107g. Hence, the correct answer is option B.
Attention NEET Students!
To make sure you are not studying endlessly, EduRev has designed NEET study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in NEET.
|
Explore Courses for NEET exam
|
|
Similar NEET Doubts
Top Courses for NEETView all
Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g?
Question Description
Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g?.
Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g?.
Solutions for Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? in English & in Hindi are available as part of our courses for NEET.
Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.
Here you can find the meaning of Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? defined & explained in the simplest way possible. Besides giving the explanation of
Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g?, a detailed solution for Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? has been provided alongside types of Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? theory, EduRev gives you an
ample number of questions to practice Some quantity of electricity is used to liberate iodine at anode and a metal at cathode.0.617g metal was deposited and iodine was completely reduced by 46.3ml of 0.124 molar sodium thiosulphate solution.what is the equivalent mass of metal ? A. 12g B. 107g C. 64g D. 38g? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET 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
|
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup