An electroplating unit deposits 3.0 g of silver onto a brass plate over a period of 3.0 minutes. Determine the current utilised by the unit. The electrochemical equivalent of silver is 1.12 × 10^ -6 kg C^ -1 .

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Quantrex Academy · Accepted Answer

Correct answer: D. 14.9 A

According to Faraday's first law of electrolysis, the mass deposited is given by

m = ZIt

, where

Z

is the electrochemical equivalent,

I

is the current, and

t

is the time.

Given:

m = 3.0 \text{ g} = 3.0 \times 10^{-3} \text{ kg}

t = 3.0 \text{ minutes} = 3.0 \times 60 \text{ s} = 180 \text{ s}

Z = 1.12 \times 10^{-6} \text{ kg C}^{-1}

Substituting the values into the formula:

I = \dfrac{m}{Zt}

I = \dfrac{3.0 \times 10^{-3}}{1.12 \times 10^{-6} \times 180}

I = \dfrac{3000}{201.6} \approx 14.9 \text{ A}

An electroplating unit deposits 3.0 g of silver onto a brass plate...

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