A. What mass of Cu is electroplated by running 13.0 A of current through a Cu^2

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

================================

Let the Time required be t sec

Therefore

(5*t)/(96500) = (48.1)/(196.966)

t = 4716.148 sec = 1.309 hours

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.