How many minutes will it take to plate out 4.50 g of Cu from a solution of Cu(NO3)2 (aq) onto the cathode of an electrolytic cel

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How many minutes will it take to plate out 4.50 g of Cu from a solution of Cu(NO3)2 (aq) onto the cathode of an electrolytic cel

l when 8.00 A of current are used? View Available Hint(s) How many minutes will it take to plate out 4.50 g of Cu from a solution of Cu(NO3)2 (aq) onto the cathode of an electrolytic cell when 8.00 A of current are used? 14.2 min 1.82 × 103 min 28.5 min 3.06 × 10−9 min Submit Return to Assignment

Chemistry

1 answer:

ipn [44] · Answer 1 · 2022-03-20T00:27:36+03:00

Answer:

It will take 28.5 minutes

Explanation:

<u>Step 1: </u>Data given

Mass of Cu = 4.50 grams

8.00 A of current are used

Molar mass of Cu = 63.5 g/mol

Step 2: Calculate time needed

Cu2+ →Electricity → Cu

we notice a flow of 2 electrons ⇒ This means the Faraday constant = 2F

Since Molar mass of Cu is 63.5 g/mol

63.5 grams of Cu is deposited by 2*96500 C

4.50 grams of Cu ((2*96500)/63.5) * 4.50 = 13677.17 C

Q = It

13677.17 = 8t*60 seconds

t = 28.5 minutes