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प्रश्न
Explain the following reaction with the balanced equation.
Zinc sulphide is heated strongly in excess of air
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उत्तर
Zinc sulphide is heated strongly in excess of air to convert it to zinc oxide. This process is called roasting.
\[\ce{\underset{\text{Zinc sulphide}}{2ZnS_{(s)}} + 3O_{2(g)} -> \underset{\text{Zinc oxide}}{2ZnO_{(s)}} + \underset{\text{Sulphur dioxide}}{2SO_2↑}}\]
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संबंधित प्रश्न
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The mixture of materials fed into a furnace to extract a metal.
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The allotrope of the non-metal carbon which conducts electricity.
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Copper reacts with nitric acid to produce nitrogen dioxide.
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Metals are malleable and ductile
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Write the name.
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Explain the concept of Roasting.
Explain in brief types of extraction of moderately reactive metals according to their reactivity.
Which of the following metals exist in their native state in nature?
(i) Cu
(ii) Au
(iii) Zn
(iv) Ag
Assertion (A): The extraction of metals from their sulphide ores cannot take place without roasting the ore.
Reason (R): Roasting converts sulphide ores directly into metals.
