Question

draw the diagram showing the electrolytic refining of copper​

Answer 1

EXPLANATION==>>

�It is the process of refining of metal in which impure metal is made the anode and a thin strip of pure metal is made the cathode. A solution of metal salt is used as an electrolyte. The apparatus is shown in the figure given below. When electric current is passed through the electrolyte, the impure metal from the anode is dissolved in the electrolyte and an equal amount of pure metal from the electrolyte is deposited on the cathode. The soluble impurities go into the solution whereas the insoluble impurities settle down at the bottom of the anode which is known as anode mud. Following diagram shows the electrolytic refining of copper in which anode is impure copper and cathode is thin strip of pure copper while the electrolyte used is the copper sulphate solution.

Answer 2

Answer:

The refining of copper takes place by electrolysis.

Explanation:

By using the electrolytic method, a metal (most commonly copper) is refined through electrolytic refining. When it comes to the mechanism of the process, electrolysis involves using a big slab or chunk of impure metal as the anode and a thin strip of pure metal as the cathode.

Step 1: Apparatus:

The anode or the positive electrode comprises the block of impure copper.

The cathode or the negative electrode comprises pure copper tubes.

Copper sulphate $\left(\mathrm{CuSO}_4\right)$ acidified with Sulphuric acid $\left(\mathrm{H}_2 \mathrm{SO}_4\right)$ acts as a graphite-coated electrolyte.

Step 2: Mechanism:

During the process of electrolysis, Copper sulphate solution dissociates into Copper ions $\left(\mathrm{Cu}^{2+}\right)$ and Sulphate ions $\left(\mathrm{SO}_4^{2-}\right)$.

There is a movement of $\mathrm{Cu}^{2+}$ ions towards the negative electrode or cathode made of pure Copper and there is an equivalent deposition of pure Copper from the electrolyte to the cathode.

The soluble impurities get dissolved into the solution while insoluble impurities get deposited at the bottom of the anode as anode mud.

Step 3: Chemical reactions involved:

At the anode, Oxidation of Copper takes place.

$\mathrm{Cu}(\mathrm{s}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-}$

At the cathode, Reduction of Copper takes place.

$\mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}(\mathrm{s})$

Hence, the refining of copper takes place by electrolysis.

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