GCSE Chemistry - Electrolysis Part 3 - Aqueous Solutions #42

The video explains electrolysis, a process of splitting compounds into elements using an electric current. It covers the setup required for electrolysis experiments and the rules for determining which ions are discharged at the electrodes. The video provides examples using copper sulphate and sodium chloride solutions, illustrating how different ions are discharged based on reactivity and presence of halides.

What is the primary requirement for ions in an electrolyte to enable electrolysis?

• They must be solid.

• They must be free to move.

• They must be in a gaseous state.

• They must be bound to a metal.

In an electrolysis experiment, where is the positive anode typically placed?

• Above the cathode

• On the right

• In the center

• On the left

Which ions are attracted to the negative cathode during electrolysis?

• Electrons

• Positive ions

• Neutral atoms

• Negative ions

According to the reactivity series, which ion is discharged at the cathode if both copper and hydrogen ions are present?

• Sodium ions

• Chloride ions

• Copper ions

• Hydrogen ions

What happens at the anode if no halide ions are present?

• Hydroxide ions are discharged.

• Sulfate ions are discharged.

• Hydrogen ions are discharged.

• Nitrate ions are discharged.

In the electrolysis of copper sulphate, what accumulates around the cathode?

• Copper metal

• Chlorine gas

• Oxygen gas

• Hydrogen gas

During the electrolysis of sodium chloride, which gas is formed at the anode?

• Nitrogen

• Chlorine

• Hydrogen

• Oxygen