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Suppose that gold is being plated onto a...

Suppose that gold is being plated onto another metal in a electrolytic cell. The half`-` cell reaction producing the `Au(s)` is `AuCl_(4)^(c-) rarr Au(s)+4Cl^(c-)+3e^(-)`
If a `0.30- A` current runs for `1.50 mi n` , what mass of `Au(s)` will be plated, assuming all the electrons are used in the reduction of `AuCl_(4)?`

A

`(0.184g)`

B

`(0.551)`

C

`(1.84g)`

D

`(0.613g)`

Text Solution

Verified by Experts

The correct Answer is:
A
Number of Faradays = `(it)/(96500) = (0.3xx15xx60)/(96500) = 2.8xx10^(-3)F`
`AuCl_(4)^(-)rightarrow Au(s) + Cl^(-) + 3e^(-)`
`3F equiv 1" mole Au "rightarrow 2.8xx10 ^(-3)F equiv (2.8)//(3) xx10^(-3)("mole") Au equiv (2.8)/(3) xx 197xx106(-3) gm Au = 0.184 gm Au`
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