Test: Electrochemistry - Year 11 MCQ

Cathode: Pb⁺ + e^- → Pb
Anode: 2Br^- → Br₂ + 2e^-

Anode: Pb²⁺ + 2e^- → Pb
Cathode: 2Br- → Br₂ + 2e^-

Cathode: Pb²⁺ + 2e^- → Pb
Anode: Br^- → Br + 2e^-

Cathode: Pb²⁺ +2e^- → Pb
Anode: 2Br^- → Br₂ + 2e^-

+ve anode -ve negode

+ve cathode -ve anode

+ve posode -ve cathode

+ve anode -ve cathode

Cathode: K⁺ + e^- → K
Anode: 2Cl^- → Cl₂ +2e^-

Cathode: 2H⁺ + 2e^- → H₂
Anode: 2Cl^- → Cl₂ + 2e^-

Cathode: H⁺ + e^- → H
Anode: 2Cl^- → Cl₂ +2e^-

Cathode: K⁺ + e^- → K
Anode: Cl^- → Cl + e^-

It can lose an electron to become a neutral atom

It can lose an electron to become a positive ion

It gains an electron to become a neutral atom

It gains an electron to become a negative ion

Copper ions at the cathode, Bromine gas at the anode

Copper metal at the anode, Bromide ions at the cathode

Copper metal at the cathode, Bromine gas at the anode

Copper metal at the anode, Bromine gas at the cathode

It completes the circuit for the flow of electrons. 

It allows ions to move between the half-cells to maintain electrical neutrality.

It prevents the electrolyte from spilling out of the cell. 

It increases the rate of reaction in the cell.

It decreases only in the anode compartment.

It increases only in the cathode compartment.

It remains constant throughout the cell.

It decreases in both compartments.

To conduct electricity into the cell 

To provide a surface for electrodeposition 

To measure the voltage of the cell 

To prevent side reactions