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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

`0.551g`

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)`
`AcCl_(4)^(c-)rarr Au(s)+Cl^(c-)+3e^(-)`
` 3F-=1 mol Au`
`implies2.8xx10^(-3)F-=(2.8)/(3)xx10^(-3) mol Au`
`-=(2.8)/(3)xx197xx10^(-3)g A u`
`=0.184 g A u`
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