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How much time would be needed to deposit...

How much time would be needed to deposite 0.25g of metallic nickel (Atomic mass = 58.5) on a metal object using a current of 1A during electroplating?

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To solve the problem of how much time is needed to deposit 0.25 g of metallic nickel using a current of 1 A during electroplating, we can follow these steps: ### Step 1: Identify the given values - Mass of nickel deposited (m) = 0.25 g - Atomic mass of nickel (M) = 58.5 g/mol - Valency of nickel (n) = +2 (since nickel typically forms +2 oxidation state) - Current (I) = 1 A - Faraday's constant (F) = 96500 C/mol ...
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