Electrochemistry

Written by Dr. Ayesha Nadeem (Chemistry)

Class 11 · Chemistry · 8 questions

Name: ____________________ Date: ____________

In a galvanic cell, oxidation takes place at the:
- A Salt bridge
- B Voltmeter
- C Cathode
- D Anode
The standard hydrogen electrode has a potential of:
- A 0 V
- B 1 V
- C -1 V
- D 0.76 V
The role of the salt bridge is to:
- A Complete the circuit by allowing ions to move
- B Cool the cell
- C Supply electrons
- D Produce hydrogen
E cell is calculated as:
- A E cathode + E anode
- B E anode - E cathode
- C E cathode - E anode
- D E cathode x E anode
Which will rust faster: iron with a zinc coating that is scratched, or iron with a tin coating that is scratched?
- A Zinc coated
- B Tin coated
- C Both equally
- D Neither
The electrode at which reduction occurs is the:
- A Wire
- B Cathode
- C Salt bridge
- D Anode
Faraday's constant is about:
- A 9650 C/mol
- B 965 C/mol
- C 96.5 C/mol
- D 96500 C/mol
The cell in a torch is a:
- A Lead acid battery
- B Solar cell
- C Fuel cell only
- D Dry cell

Answer key

1. D, 2. A, 3. A, 4. C, 5. B, 6. B, 7. D, 8. D

Oxidation occurs at the anode in all cells.
It is defined as 0.00 V.
It lets ions flow and keeps the half cells neutral.
Use standard reduction potentials: E cell = E cathode - E anode.
Zinc is more reactive and protects the iron. Tin is less reactive, so exposed iron corrodes.
Reduction occurs at the cathode.
One mole of electrons carries about 96500 C.
The zinc carbon dry cell is common in torches.