A. What mass of Cu is electroplated by running 13.0 A of current through a Cu^2
ID: 632664 • Letter: A
Question
A. What mass of Cu is electroplated by running 13.0 A of current through a Cu^2 solution for 4.00 h? Express your answer to three significant figures and include the appropriate units. B. How many minutes will it take to electroplate 48.1g of gold by running 5.00 A of current through a solution of Au+? Express your answer to three significant figures and include the appropriate units please show work so i can learn. A. What mass of Cu is electroplated by running 13.0 A of current through a Cu^2 solution for 4.00 h? Express your answer to three significant figures and include the appropriate units. B. How many minutes will it take to electroplate 48.1g of gold by running 5.00 A of current through a solution of Au+? Express your answer to three significant figures and include the appropriate units please show work so i can learn.Explanation / Answer
Here
Q = It
= 13*4*60*60
= 187200 C
Now 96500 C is required for 1 equivalent mass
Here
No. of Equivalents deposit = (187200/96500)
= 1.939
Therefore
Mass Deposit = 1.939*0.5*63.5
= 61.563 g
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Let the Time required be t sec
Therefore
(5*t)/(96500) = (48.1)/(196.966)
t = 4716.148 sec = 1.309 hours