A current of 0.15 A is passed through an aqueous solution of K2PtCl4. How long will it take to deposit 1.00 g Pt (s) (M = 195.1) ?

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Chemistry

Bailey Schultz

1 November, 05:39

A current of 0.15 A is passed through an aqueous solution of K2PtCl4. How long will it take to deposit 1.00 g Pt (s) (M = 195.1) ?

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Cheeky · Answer 1

First calculate the electric charge used to deposit 1.0 g Pt

C = (1.0 g Pt) (1 mol Pt / 195.1 g Pt) (2 mol e / 1 mol Pt) (96485 C / 1 mol e)

C = 989.08 C

C = It

Where I is the current

T is the time

T = C / i

T = 989.08 C / 0.15 A

T = 6593.88 s

T = 1.83 hrs