Open Question
Sketch the galvanic cell and determine the line notation for the following redox reaction:
Ni2+ (aq) + Mg (s) ⇌ Ni (s) + Mg 2+ (aq)
13. Fundamentals of Electrochemistry
Electrochemical Cells
Struggling with Analytical Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Calculate the standard cell potential (E°cell) for the galvanic cell based on the following reaction: Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s). Given: E°(Zn^2+/Zn) = -0.76 V, E°(Cu^2+/Cu) = +0.34 V.
A
+0.42 V
B
+1.10 V
C
-1.10 V
D
-0.42 V
Verified step by step guidance1
Identify the half-reactions involved in the galvanic cell. For the given reaction, the oxidation half-reaction is Zn(s) → Zn^2+(aq) + 2e^- and the reduction half-reaction is Cu^2+(aq) + 2e^- → Cu(s).
Determine the standard reduction potentials (E°) for each half-reaction. From the problem, E°(Zn^2+/Zn) = -0.76 V and E°(Cu^2+/Cu) = +0.34 V.
Understand that the standard cell potential (E°cell) is calculated using the formula: E°cell = E°(cathode) - E°(anode). Here, the cathode is where reduction occurs (Cu^2+/Cu), and the anode is where oxidation occurs (Zn^2+/Zn).
Substitute the values into the formula: E°cell = E°(Cu^2+/Cu) - E°(Zn^2+/Zn). This becomes E°cell = +0.34 V - (-0.76 V).
Perform the arithmetic operation to find the standard cell potential. The result will give the E°cell value for the galvanic cell.
5:40mWatch next
Master Galvanic or Voltaic Cell with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Electrochemical Cells practice set
Problem sets built by lead tutorsExpert video explanations