1. Tardigrade
  2. Question
  3. Chemistry
  4. Suppose that gold is being plated on to another metal in an electrolytic cell. The half-cell reaction producing the Au ( s ) is AuCl 4 - arrow Au (s)+4 Cl --3 e- If a 0.30 A current runs for 15.00 min, what mass of Au (s) will be plated, assuming all the electrons are used in the reduction of AuCl 4-? The Faraday constant is 96485 C / mol and molar mass of Au is 197 .

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Q. Suppose that gold is being plated on to another metal in an electrolytic cell. The half-cell reaction producing the $Au ( s )$ is $AuCl _{4}{ }^{-} \rightarrow Au (s)+4 Cl ^{-}-3 e^{-}$ If a $0.30\, A$ current runs for $15.00\, \min$, what mass of $Au (s)$ will be plated, assuming all the electrons are used in the reduction of $AuCl _{4}^{-}$? The Faraday constant is $96485\, C / mol$ and molar mass of $Au$ is $197$ .

ManipalManipal 2014Electrochemistry

Solution:

Mass of $Au$ deposited $=$ Number of Faraday passed $\times$ Eq. mass
$=\frac{0.30 \times 15 \times 60}{96485} \times \frac{197}{3}$
$=0.184\, g$