Calculate the mass of Cu (AM: 63.5) produced by passing 5.00 A through molten Cu

Question

Calculate the mass of Cu (AM: 63.5) produced by passing 5.00 A through molten CuSO_4 foe 2.00 h. At what electrode is Cu produced? (F = 96485 C/mol) Give signs (+, -, or 0) for Delta H degree, Delta S degree, Delta G degree, and w_pv for the reaction, H_2O(g) rightarrow H_2O(l) at 25 degree C, 1 aim. Given the vaporization of bromine at 25 degree C, 1 atm, Br_2(l) rightarrow Br_2(g) Delta H degree = 30.71 kJ, Delta S degree = 93.0 J/K a) W_pv. Is work done by or to the system? (R = 8.314 J/mol middot K)

Explanation / Answer

7. When current is passed through CuSO4, electrolysis takes place i.e Cu2+ ions are liberated at anode and deposited at cathode. So Cu is produced at cathode.

Cathode(reduction):Cu2++2e-=Cu

Anode (oxidation):Cu=Cu2++2e-

Mass of Cu produced=m=ZIt

Where Z= Electrochemical equivalent=M/96500q(M=molar mass)

I= current= 5A

t=time in seconds=2×3600

Putting values in above equation

m=(63.5×7200×5)÷(96500×2)=11.85g

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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