At a current strength of 5A, zinc with a mass of 1.017g was released in the electrolytic

At a current strength of 5A, zinc with a mass of 1.017g was released in the electrolytic bath in 10 minutes. Determine the electrochemical equivalent of zinc.

To determine the desired electrochemical equivalent of zinc, we apply the first Faraday’s law: m = k * I * t and k = m / (I * t).

Values of variables: I – current strength (I = 5 A); t is the duration of zinc evolution (t = 10 min; in SI t = 600 s); m is the mass of the zinc obtained (m = 1.017 g; in SI m = 1.017 * 10-3 kg).

Let’s calculate: k = m / (I * t) = 1.017 * 10-3 / (5 * 600) = 0.339 * 10-6 kg / Cl.

Answer: The electrochemical equivalent of zinc, according to the calculation, is 0.339 * 10-6 kg / C.