Can I have help?

Question

How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for 1.55 h? (F = 96,500 C/mol)

Answer 1

Cu²⁺(aq) + 2e- ==> Cu(s)

1 A (amp) = 1 C/s (1 coulomb per second)

1 mol electrons = 96,500 coulomb

2.50 A = 2.50 C/s

1.55 h = 1.55 h x 60 min / h x 60 sec / min = 5580 sec

2.50 C/s x 5580 s = 13,950 C

13,950 C x 1 mol e- / 96,500 C = 0.1446 moles e-

0.1446 mol e- x 2 mol e- / mol Cu = 0.289 mol Cu deposited

0.289 mol Cu x 63.55 g / mol = 18.4 g Cu deposited

(be sure to check the math)