During electrolysis, 500 mg of silver was released from an aqueous solution of silver salt.

During electrolysis, 500 mg of silver was released from an aqueous solution of silver salt. What charge went through the electrolytic bath? The electrochemical equivalent of silver is 1.12 × 10 ^ -6 kg / C

To calculate the charge passed through the electrolytic bath, we use Faraday’s law: m = k * I * Δt = k * q, whence we express: q = m / k.

Constants and variables: m is the mass of released silver (m = 500 mg = 5 * 10-4 kg); k is the electrochemical equivalent of silver (according to the condition k = 1.12 * 10-6 kg / C).

Let’s make a calculation: q = m / k = 5 * 10-4 / (1.12 * 10-6) = 446.43 Cl.

Answer: A charge of 446.43 C had to pass through the electrolytic bath.