Explanation of the volume of gas collected over one electrode being double than that of gas collected over the other electrode in the electrolysis of water:

Electrolysis of Water:
- Electrolysis of water involves passing an electric current through water to separate it into its constituent elements, hydrogen and oxygen gas.

Formation of Hydrogen and Oxygen Gas:
- At the anode (positive electrode), oxygen gas is produced through the oxidation of water molecules.
- 2H2O(l) -> O2(g) + 4H+(aq) + 4e-
- At the cathode (negative electrode), hydrogen gas is produced through the reduction of water molecules.
- 2H2O(l) + 2e- -> H2(g) + 2OH-(aq)

Volume of Gas Collected:
- Since each water molecule consists of two hydrogen atoms and one oxygen atom, the volume ratio of hydrogen gas to oxygen gas produced is 2:1.
- This means that for every volume of oxygen gas collected at the anode, double the volume of hydrogen gas is collected at the cathode.

Explanation:
- The reason for the double volume of hydrogen gas collected compared to oxygen gas is due to the stoichiometry of the reaction.
- For every oxygen molecule produced, two hydrogen molecules are produced, leading to a double volume of gas collected over one electrode compared to the other.

Overall Reaction:
- The overall reaction for the electrolysis of water is:
2H2O(l) -> 2H2(g) + O2(g)
- This reaction shows that for every volume of oxygen gas produced, double the volume of hydrogen gas is produced, explaining why the volume of gas collected over one electrode is double than that collected over the other electrode.