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Production Process of Sodium Sulfide (Na₂S) Sodium Sulphate
Na₂SO₄ is fed into a hopper via an automatic feeder and then conveyed into a combustion chamber, where Sodium Sulphate is blown and burned using coal gas. When the temperature reaches 884°C, sodium sulfate melts into a liquid state. The dissolved Na₂SO₄ becomes chemically unstable, and the SO₄²⁻ ions are readily decomposed. A chemical substitution reaction occurs using carbon monoxide from phosphorous-containing coal gas, as follows:
Na₂SO₄ + 4CO → Na₂S + 4CO₂
When the flame in the furnace changes from blue to red, the substitution reaction by CO is complete. Beyond this point, CO serves only as a fuel to further increase the temperature. When the temperature reaches 1100°C, a small amount of anthracite is added. The reaction endpoint is indicated by the appearance of a yellow sparkling flame inside the furnace. The chemical reaction is as follows:
Na₂SO₄ + 2C → Na₂S + 2CO₂
Sodium Sulphate.