Cyanide Process

Cyanide process is also called as Macarthur-forest Process. It is the process of extracting gold or silver from the ores by dissolving in a dilute solution of potassium cyanide or sodium cyanide. This process was introduced in the year 1887 by the Scottish chemists naming Robert W. Forrest, John S. MacArthur, and William Forrest.

This method involves three steps- In the first step, the finely ground ore is contacted with the solution containing the cyanide, the second step involves the seperating of solids from the clear solution and the third step involves the recovery of precious metals from solution by precipitating with the zinc dust.

Cyanide Process – Extraction of Gold through cyanidation

Gold is usually found in low concentration in the form of ore which is mined. Gold should be separated from other minerals present in the ore. As gold is insoluble, it should be separated
from other minerals to make it soluble. Hence, sodium cyanide can be added, where cyanide ions form a complex ion with the molecules of gold.

The cyanide process is as explained below-

• The ore is grounded and crushed. If the ore containing the gold has other form of metals or any kind of sulphide minerals then it requires additional kind of treatments before going through the process of leaching. The gold is mixed with the sodium cyanide which leads to the following Elsener’s equation and reaction. This is done to make soluble gold
• Now the gold is soluble. This method of making soluble gold is known as leaching. In the process of leaching, dilute form of sodium cyanide is added into the ore containing the gold. Since gold is soluble after leaching process, it is free to move through membrane while the rest of ore cannot pass through the membrane. Lime is added to sodium cyanide to make the pH in between 10-11 so as to favor the reactants and bring them to equilibrium.
• The slurry formed is treated with activated zinc or carbon for the extraction of gold. Cementation is next process which involves the use of zinc electrode in paste of carbon immersed in the solution containing the gold cyanide.

The following reactions occur-

At Cathode –  $e^{-} + Au(CN)_{2}]^{-}\rightarrow Au + 2CN^{-}$

Gold is thus reduced gaining electrons or by the decrease in the oxidation number

At Anode – $Zn + 2OH^{-}\rightarrow Zn(OH)_{2} + 2e^{-}$

Zinc is next oxidised to lose electrons or by increase in the oxidation number

$Zn(OH)_{2} + 4CN^{-}\rightarrow Zn(CN)_{4}^{2-} + 2OH^{-}$

The cyanide remaining in the tailings. I.e the slurry obtained after the process of gold leaching needs to be recycled or destroyed in some way.

Practise This Question

Find the value of 163÷43.