If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion?

how would you work this out?

thanks.:)

Question

If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion?

how would you work this out?

thanks.:)

Pankaj · Answer

Using Farady's First Law of Electrolysis.

m = ZIt

or

z = m/It = 863000/ (1.47)(525) =1118.16

Charge on metal ion = 1118.16 x1.60217657 × 10-19coulombs

Thanks & Regards

Pankaj Singh

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If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion? how would you work this out? thanks.:)

If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion?

how would you work this out?

thanks.:)

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If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion? how would you work this out? thanks.:)

If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion? how would you work this out? thanks.:)

1 Answers

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If 1.47 A of current was passed through an aqueous solution of a metal salt for 525 seconds and 863 mg of metal was deposited, then what was the charge on metal ion?

how would you work this out?

thanks.:)