A strip of copper is placed in a beaker with a 1.0 M solution of Cu(NO3)2. A str

Question

A strip of copper is placed in a beaker with a 1.0 M solution of Cu(NO3)2. A strip of silver is placed in a second beaker with A 1.0 M solution of AgNO3. A salt bridge connects the two beakers and the two metal electrodes are connected by wires to a digital voltmeter. The voltmeter reads 0.46 V. Which reaction is occurring at the anode and which reaction is occurring at the cathode? Note: In this cell, the standard reduction potential for Ag | Ag+ is + 0.80 V and the standard reduction potential for Cu | Cu2+ is + 0.34 V

Explanation / Answer

As silver has a higher reduction potential than copper, silver will be the one that reduces, or, the one that occurs in the cathode. Hence, copper wil oxidize in the anode.

Answer is letter a).

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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