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प्रश्न
Explain the following reaction with the balanced equation.
Zinc oxide is treated with carbon
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उत्तर
Zinc oxide is reduced to zinc by heating it with carbon.
\[\ce{\underset{\text{Zinc oxide}}{ZnO_{(s)}} + \underset{\text{Carbon}}{C_{(s)}} ->[Heat] \underset{\text{Zinc}}{Zn_{(s)}} + \underset{\text{Carbon monoxide}}{CO↑}}\]
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संबंधित प्रश्न
Give reasons.
Aluminium is a highly reactive metal, yet it is used to make utensils for cooking.
Why are the metals like Na, K, Ca and Mg never found in their free state in nature?
Which one of the methods given in column I is applied for the extraction of each of the metals given in column II:
| Column I | Column II |
| Electrolytic reduction | Aluminium |
| Reduction with Carbon | Zinc |
| Reduction with Aluminium | Sodium |
| Iron | |
| Manganese | |
| Tin |
Define the term mineral.
Define the term gangue.
Explain giving equation, what happens when:
A mixture of Cu2O and Cu2S is heated.
Which gas is produced during the extraction of aluminium? At which electrode is this gas produced?
During galvanisation, iron metal is given a thin coating of one of the following metals. This metal is:
Aluminum is used in thermite welding:
what is thermit?
Name the anode, the cathode and the electrolyte used in the electrolytic refining of impure copper.
Name the following:
The mixture of materials fed into a furnace to extract a metal.
Name the following:
The process of heating a substance very strongly in such a way that it does not combine with oxygen.
How many valence electrons are present in metals ?
To protect iron from rusting, it is coated with a thin layer of zinc. Name the process.
Correct the following statement :
Copper reacts with nitric acid to produce nitrogen dioxide.
Choose the correct answer from the options given below:
The metal is a liquid at room temperature.
Define roasting.
Carbon cannot reduce the oxides of sodium, magnesium, and aluminum to their respective metals. Why? Where are these metals placed in the reactivity series? How are these metals obtained from their ores? Take an example to explain the process of extraction along with chemical equations.
Identify who I am!
Ore of Aluminum- ______
On the basis of reactivity metals are grouped into three categories:
- Metals of low reactivity
- Metals of medium reactivity
- Metals of high reactivity
Therefore metals are extracted in pure form from their ores on the basis of their chemical properties.
Metals of high reactivity are extracted from their ores by electrolysis of the molten ore.
Metals of low reactivity are extracted from their sulphide ores, which are converted into their oxides. The oxides of these metals are reduced to metals by simple heating.
(a) Name the process of reduction used for a metal that gives vigorous reaction with air and water both.
(b) Carbon cannot be used as a reducing agent to obtain aluminium from its oxide? Why?
(c) Describe briefly the method to obtain mercury from cinnabar. Write the chemical equation for the reactions involved in the process.
OR
(c) Differentiate between roasting and calcination giving chemical equation for each.
