Determine the quantity indicated for each of the following electrolyses. Enter s

Question

Determine the quantity indicated for each of the following electrolyses.

Enter scientific notation as 1.23E4.

(a) [Cu2+] remaining in 429 mL of a solution that was originally 0.569 M CuSO4, after passage of 3.91 A for 605 s and the deposition of Cu at the cathode. (Note: 1 A = 1 C s–1) DO NOT ANSWER A) AS I GOT THE CORRECT ANSWER AS 0.541M.

0.541 M

(b) The time required to reduce [Ag+] in 354 mL of AgNO3(aq) from 0.159 to 0.147 M by electrolyzing the solution between Pt electrodes with a current of 4.23 A. (Note: 1 A = 1 C s–1)

FOR PART B, I GOT ANSWER AS 98.1 SECONDS. THIS IS INCORRECT. HERE IS THE FEEDBACK I HAVE RECEIVED

There are 2 moles of electrons consumed for every 1 mole of Cu deposited, and 1 mole of electrons consumed for every 1 mole of Ag deposited.

PLEASE CALUCLATE PART B CORRECTLY. THANK YOU

There are 2 moles of electrons consumed for every 1 mole of Cu deposited, and 1 mole of electrons consumed for every 1 mole of Ag deposited.

PLEASE CALUCLATE PART B CORRECTLY. THANK YOU

Explanation / Answer

(b) moles of Ag deposited = (0.159 - 0.147) M x 0.354 L = 4.248 x 10^-3 mols

time required to deposit this much Ag = 4.248 x 10^-3 x 96485/4.23 = 96.90 s

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