How hydrogen on large scale is prepared from water?

How SODIUM METAL on large scale is prepared from common salt?

Look up electrolysis.

For both questions?

To prepare hydrogen on a large scale from water, a process called electrolysis is commonly used. Here's how it works:

1. First, water is added to an electrolysis cell, which consists of two electrodes, usually made of metal such as platinum or graphite, submerged in the water.

2. A direct current (DC) power source is connected to the electrodes. The positive terminal (anode) of the power source is connected to the electrode where oxygen will be produced, and the negative terminal (cathode) is connected to the electrode where hydrogen will be produced.

3. When the electric current flows through the water, it causes electrolysis to occur. This means that water molecules are split apart into their component elements: hydrogen and oxygen.

4. At the cathode, hydrogen gas (H2) is formed through the reduction reaction: 2H2O + 2e- → H2 + 2OH-

5. At the anode, oxygen gas (O2) is formed through the oxidation reaction: 4OH- → 2H2O + O2 + 4e-

6. The hydrogen gas is collected and stored for various applications, such as fuel cell technology or chemical synthesis.

Now let's discuss how sodium metal is prepared on a large scale from common salt (sodium chloride):

1. The main industrial method for sodium metal production is the Downs process. This process involves the electrolysis of a molten sodium chloride (NaCl) solution.

2. A large electrolysis cell is designed to withstand high temperatures. The cell is first heated to approximately 600-700°C, which ensures that the sodium chloride is melted.

3. Next, a graphite anode and a steel cathode are introduced to the molten sodium chloride. The anode and cathode are connected to an external power supply, such as a DC power source.

4. When the power supply is turned on, an electric current passes through the molten sodium chloride. Electrolysis takes place, resulting in the decomposition of sodium chloride.

5. At the cathode, sodium ions receive electrons and are reduced to form sodium metal (Na): Na+ + e- → Na

6. At the anode, chloride ions lose electrons and are oxidized to form chlorine gas (Cl2): 2Cl- → Cl2 + 2e-

7. The sodium metal sinks to the bottom of the electrolysis cell, as it is denser than the molten salt. It can be collected and further processed for industrial uses.

So, in summary, hydrogen on a large scale is prepared from water using the electrolysis process, while sodium metal on a large scale is prepared from common salt (sodium chloride) through the Downs process, which involves molten electrolysis.