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Why does the electrolytic reduction of the metals in group 1 and 2 proceed under molten salt conditions?
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∙ 10y ago
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∙ 10y ago
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What method do we use to extract more reactive metals such as aliminium?
Through electrolytic reduction.
How are redox reactions used to obtain pure metals?
One way is electrolytic reduction of metal cations from molten salts. Another is heating with carbon, which can reduce the metal ions in many metal oxides to elemental metal atoms.
What is the standard reduction potential E?
This is a table with values in volts for the standard reduction potentials of metals to a cathode.
What is a reduction potential chart?
This is a table with values in volts for the standard reduction potentials of metals to a cathode.
What is reduction of non metals?
Reduction means a gain of electrons, which is what non-metals do in order to observe the "octet rule." For example, elemental chlorine has an oxidation number of 0. When chlorine gains an electron, it forms a -1 charged ion, so its oxidation number is now -1. From 0 to -1 is a numerical reduction, which is why it's called that.
What method do we use to extract more reactive metals such as aliminium?
Through electrolytic reduction.
What is the difference between electrolytic reduction and electrolytic refining under these heads a. electrodes b. electrolytes c. reaction at positive and negative electrodes?
The difference between electrolytic refining and electrolytic reduction is as follows: a. In electrolytic reduction graphite electrodes are used which are of same size. in electrolytic refining the anode is made of the impure metal which is to be purified and the cathode is made from that pure metal. initially the cathode is thick and the anode is very thin. b. the electrolyte used in electrolytic refining is the metal sulphate with acid (acid id added to increase the conductivity) which is aqueous in nature. whereas in electrolytic reduction molten chloride form of the solution is used. c. The impure metal at the anode displaces the metal from the aqueous solution and the these ions go to the cathode and attach to the cathode as they are now pure. basically the impure metal at the anode directly doesn't go to the cathode, its a indirect process. as the reaction goes on, the size of the anode reduces and finally disappears and the cathode becomes thick as all the impure metal is converted into pure metal. this happens in electrolytic refining. whereas in electrolytic reduction the metal from the molten solution deposits on the cathode and chlorine gas is evolved at the anode. general differences: a. in electrolytic reduction no anode mud is formed and in electrolytic refining anode mud is formed from the impurities oh the impure metal. b. electrolytic reduction is done to extract metals of high reactivity from their ores. electrlolytic refining is done to purify (refine) metals from their impure form.
How are redox reactions used to obtain pure metals?
One way is electrolytic reduction of metal cations from molten salts. Another is heating with carbon, which can reduce the metal ions in many metal oxides to elemental metal atoms.
Should oxidation or reduction be done to extract metals from their compounds?
A reduction reaction is frequently used to obtain pure metals.
What is the standard reduction potential E?
This is a table with values in volts for the standard reduction potentials of metals to a cathode.
What is a reduction potential chart?
This is a table with values in volts for the standard reduction potentials of metals to a cathode.
Why is carbon reduction process not applicable for reduction of oxides of metals like Mn and Cr?
carbon can not reduce more electropositive metallic oxides like of Mn and Cr. Thus carbon reduction process not applicable for reduction of oxides of metals like Mn and Cr .
What has the author P V Shigolev written?
P. V. Shigolev has written: 'Electrolytic and chemical polishing of metals'
How many ways of making metals?
by electrolysis by thermal reduction
What type of chemical reaction is used to extract metals from their naturallly occurring compounds like oxides or chlorides?
For example reduction with hydrogen and carbon from oxides, reduction with other metals from chlorides, etc.
What metal oxides can be converted to the metal by carbon reduction but not by hydrogen reduction?
any metals below carbon in the reactivity series. :)
Why can the active metals in groups 1 and 2 in the periodic table not be reduced in aqueous electrolytic cells?
The active metals in columns 1 and 2 of a wide form periodic table cannot be reduced to elemental metals by electrolysis in aqueous electrolytic cells, because any atom of elemental active metal that might be transiently produced, by reduction of a positive ion of the active metal to a neutral atom, will react almost instantaneously with two nearby water molecules to produce hydrogen gas, hydroxyl ions, and regenerated positive ions of the active metal.
