Question

electrochemical equivalent of a substance is 0.0006 its equivalent weight is

Answer 1

57.9

Answer 2

• Concept: Faraday's first law of electrolysis states that the mass (W) of a substance deposited or liberated at an electrode is directly proportional to the quantity of electricity (Q) passed through the electrolyte:

  $W = ZQ$

  where Z is the electrochemical equivalent.

• Relationship between Electrochemical Equivalent (Z) and Equivalent Weight (E): One Faraday (F) of electricity (approximately 96500 Coulombs) deposits or liberates one equivalent weight (E) of a substance.

  Therefore, if Q = F, then W = E.

  Substituting this into the formula:

  $E = Z \times F$

• Given values:

  Electrochemical equivalent (Z) = 0.0006 g/C

  Faraday's constant (F) = 96500 C/mol

• Calculation:

  $E = 0.0006 \, \text{g/C} \times 96500 \, \text{C/mol}$

  $E = 57.9 \, \text{g/mol}$

The equivalent weight of the substance is 57.9.

Explanation of the solution:

The electrochemical equivalent (Z) is the mass of a substance deposited by one coulomb of charge. The equivalent weight (E) is the mass of a substance deposited by one Faraday (F) of charge. Since 1 Faraday = 96500 Coulombs, the relationship is $E = Z \times F$. Substituting the given Z = 0.0006 g/C and F = 96500 C/mol, we get $E = 0.0006 \times 96500 = 57.9$ g/mol.