Answer: 116 g of copper
Explanation:
[tex]Q=I\times t[/tex]
where Q= quantity of electricity in coloumbs
I = current in amperes = 24.5A
t= time in seconds = 4.00 hr = [tex]4.00\times 3600s=14400s[/tex] (1hr=3600s)
[tex]Q=24.5A\times 14400s=352800C[/tex]
[tex]Cu^{2+}+2e^-\rightarrow Cu[/tex]
[tex]2\times 96500C=193000C[/tex] of electricity deposits 63.5 g of copper.
352800 C of electricity deposits = [tex]\frac{63.5}{193000}\times 352800=116g[/tex] of copper.
Thus 116 g of Cu(s) is electroplated by running 24.5A of current
Thus remaining in solution = (0.1-0.003)=0.097moles
