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A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal?
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A current of 5 ampere is passed through an electrolyte for 15 minutes ...
To calculate the electrochemical equivalent (E) of the metal deposited from an electrolyte, we can use Faraday's laws of electrolysis. Here’s a step-by-step breakdown of the calculation:
Given Data:
- Current (I) = 5 A
- Time (t) = 15 minutes = 15 × 60 seconds = 900 seconds
- Mass of metal deposited (m) = 3 g
Formula for Electrochemical Equivalent:
- The electrochemical equivalent (E) is calculated using the formula:
\[
E = \frac{m}{Q}
\]
where \( Q \) is the total electric charge passed through the electrolyte.
Calculating Total Charge (Q):
- The total charge (Q) can be calculated using the formula:
\[
Q = I \times t
\]
Substituting the values:
\[
Q = 5 \, \text{A} \times 900 \, \text{s} = 4500 \, \text{C}
\]
Calculating Electrochemical Equivalent (E):
- Now substituting the values of \( m \) and \( Q \) into the equation for E:
\[
E = \frac{3 \, \text{g}}{4500 \, \text{C}} = \frac{3}{4500} \, \text{g/C} = 0.0006667 \, \text{g/C}
\]
Final Result:
- Therefore, the electrochemical equivalent of the metal is:
\[
E \approx 0.00067 \, \text{g/C}
\]
This value indicates the mass of the metal deposited per coulomb of charge passed through the electrolyte.
Given Data:
- Current (I) = 5 A
- Time (t) = 15 minutes = 15 × 60 seconds = 900 seconds
- Mass of metal deposited (m) = 3 g
Formula for Electrochemical Equivalent:
- The electrochemical equivalent (E) is calculated using the formula:
\[
E = \frac{m}{Q}
\]
where \( Q \) is the total electric charge passed through the electrolyte.
Calculating Total Charge (Q):
- The total charge (Q) can be calculated using the formula:
\[
Q = I \times t
\]
Substituting the values:
\[
Q = 5 \, \text{A} \times 900 \, \text{s} = 4500 \, \text{C}
\]
Calculating Electrochemical Equivalent (E):
- Now substituting the values of \( m \) and \( Q \) into the equation for E:
\[
E = \frac{3 \, \text{g}}{4500 \, \text{C}} = \frac{3}{4500} \, \text{g/C} = 0.0006667 \, \text{g/C}
\]
Final Result:
- Therefore, the electrochemical equivalent of the metal is:
\[
E \approx 0.00067 \, \text{g/C}
\]
This value indicates the mass of the metal deposited per coulomb of charge passed through the electrolyte.
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A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal?
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A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal?.
A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A current of 5 ampere is passed through an electrolyte for 15 minutes when 3 gm of a metal was deposited. Calculate the electrochemical equivalent of the metal?.
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