When one coulomb of electricity is passed through an electrolytic solution, the mass of the element deposited on the electrode is equal to

Options

A. Molecular weight
B. equivalent weight
C. one gram
D. Electrochemical equivalent

Answer

To determine the mass of the element deposited on the electrode when one coulomb of electricity is passed through an electrolytic solution, we can use the concept of electrochemical equivalent (ECE). Here are the step-by-step calculations:

### Step 1: Understand the Concept of Electrochemical Equivalent (ECE)
The electrochemical equivalent (ECE) is defined as the mass of a substance deposited or liberated at an electrode when one coulomb of electric charge is passed through an electrolytic solution.

### Step 2: Use the Formula for Electrochemical Equivalent
The formula for calculating the mass (m) of the substance deposited is given by:
\[ m = \frac{Q \cdot E}{F} \]
Where:
- \( m \) = mass of the substance deposited (in grams)
- \( Q \) = charge passed (in coulombs)
- \( E \) = electrochemical equivalent (in grams per coulomb)
- \( F \) = Faraday's constant (approximately \( 96485 \, C/mol \))

### Step 3: Substitute the Values
In this case, we are passing \( Q = 1 \, C \) of charge. The electrochemical equivalent \( E \) can vary depending on the substance being deposited, but for the sake of this question, we can denote it as \( E \).

Thus, substituting into the formula:
\[ m = \frac{1 \cdot E}{F} \]

### Step 4: Simplify the Equation
Since we are interested in the mass deposited when 1 coulomb of charge is passed, we can express it as:
\[ m = \frac{E}{F} \]

### Step 5: Conclusion
The mass of the element deposited on the electrode when one coulomb of electricity is passed through the electrolytic solution is equal to \( \frac{E}{F} \), where \( E \) is the electrochemical equivalent of the element in grams per coulomb.