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 AuCl4-+3e- arrow Au(s)+4(Cl)- . If a 0.30A current passed for 15min , what mass of Au(.s.) will be plated, assume all the electrons are used in the reduction of AuCl4- ? The Faraday constant is 96485C/mol and molar mass of Au textis197 .

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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 $Au\left(\right.s\left.\right)$ is $AuCl_{4}^{-}+3e^{-} \rightarrow Au\left(s\right)+4\left(Cl\right)^{-}$ . If a $0.30A$ current passed for $15min$ , what mass of $Au\left(\right.s\left.\right)$ will be plated, assume all the electrons are used in the reduction of $AuCl_{4}^{-}$ ?
The Faraday constant is $96485C/mol$ and molar mass of $Au\text{is}197$ .

NTA AbhyasNTA Abhyas 2022

Solution:

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