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? 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

It will take 28.5 minutes

Explanation:

Step 1: 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

the answer is:  

line graphs show patterns in data with variables that change over time; whereas, circle graphs show data as parts out of a whole (such as out of 100%).