NEET Exam > NEET Questions > How many grams of silver could be plated out ...
Start Learning for Free
How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)?
Most Upvoted Answer
How many grams of silver could be plated out on a serving tray by pass...
Community Answer
How many grams of silver could be plated out on a serving tray by pass...
Solution:
Given data:
Time, t = 8 hours = 8 x 3600 s
Current, I = 9 A
Atomic mass of Ag = 107.8 g/mol
Density of Ag = 10 g/cm³
Thickness of silver plating, d = 0.002 cm
Step 1: Calculation of the amount of charge passed
The amount of charge passed, Q = I x t
Q = 9 A x 8 x 3600 s
Q = 2.592 x 10⁵ C
Step 2: Calculation of the amount of Ag deposited
From Faraday's law of electrolysis, the amount of Ag deposited is given by:
m = (Q x M) / (n x F)
where,
m = mass of Ag deposited (in grams)
Q = amount of charge passed (in coulombs)
M = atomic mass of Ag (in grams/mole)
n = number of electrons required for the reduction of one Ag+ ion (1 electron in this case)
F = Faraday constant (96,485 C/mol)
Substituting the values, we get:
m = (2.592 x 10⁵ C x 107.8 g/mol) / (1 x 96,485 C/mol)
m = 287.9 g
Therefore, 287.9 g of Ag can be plated out on the serving tray.
Step 3: Calculation of the area of the tray
The volume of the Ag deposited is given by:
V = m / ρ
where,
V = volume of Ag deposited (in cm³)
m = mass of Ag deposited (in grams)
ρ = density of Ag (in g/cm³)
Substituting the values, we get:
V = 287.9 g / 10 g/cm³
V = 28.79 cm³
The area of the tray can be calculated using the formula:
V = A x d
where,
A = area of the tray (in cm²)
d = thickness of the silver plating (in cm)
Substituting the values, we get:
28.79 cm³ = A x 0.002 cm
A = 14,395 cm²
Therefore, the area of the tray is 14,395 cm².
Conclusion:
Thus, 287.9 g of Ag can be plated out on the serving tray by passing electrolysis of a solution of Ag(1) salt for 8 hours at a current of 9 ampere. The area of the tray is 14,395 cm² if the thickness of the silver plating is 0.002 cm.
Given data:
Time, t = 8 hours = 8 x 3600 s
Current, I = 9 A
Atomic mass of Ag = 107.8 g/mol
Density of Ag = 10 g/cm³
Thickness of silver plating, d = 0.002 cm
Step 1: Calculation of the amount of charge passed
The amount of charge passed, Q = I x t
Q = 9 A x 8 x 3600 s
Q = 2.592 x 10⁵ C
Step 2: Calculation of the amount of Ag deposited
From Faraday's law of electrolysis, the amount of Ag deposited is given by:
m = (Q x M) / (n x F)
where,
m = mass of Ag deposited (in grams)
Q = amount of charge passed (in coulombs)
M = atomic mass of Ag (in grams/mole)
n = number of electrons required for the reduction of one Ag+ ion (1 electron in this case)
F = Faraday constant (96,485 C/mol)
Substituting the values, we get:
m = (2.592 x 10⁵ C x 107.8 g/mol) / (1 x 96,485 C/mol)
m = 287.9 g
Therefore, 287.9 g of Ag can be plated out on the serving tray.
Step 3: Calculation of the area of the tray
The volume of the Ag deposited is given by:
V = m / ρ
where,
V = volume of Ag deposited (in cm³)
m = mass of Ag deposited (in grams)
ρ = density of Ag (in g/cm³)
Substituting the values, we get:
V = 287.9 g / 10 g/cm³
V = 28.79 cm³
The area of the tray can be calculated using the formula:
V = A x d
where,
A = area of the tray (in cm²)
d = thickness of the silver plating (in cm)
Substituting the values, we get:
28.79 cm³ = A x 0.002 cm
A = 14,395 cm²
Therefore, the area of the tray is 14,395 cm².
Conclusion:
Thus, 287.9 g of Ag can be plated out on the serving tray by passing electrolysis of a solution of Ag(1) salt for 8 hours at a current of 9 ampere. The area of the tray is 14,395 cm² if the thickness of the silver plating is 0.002 cm.
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
How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)?
Question Description
How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)?.
How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)?.
Solutions for How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? 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 How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? defined & explained in the simplest way possible. Besides giving the explanation of
How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)?, a detailed solution for How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? has been provided alongside types of How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? theory, EduRev gives you an
ample number of questions to practice How many grams of silver could be plated out on a serving tray by passing electrolysis of a solution of Ag (1) salt for 8 hours at a current of 9 ampere? What is the area of the tray, if thickness of the silver platting is 0.002cm? Density of silver is 10g/cm^3.( Atomic mass of Ag=107.8)? 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