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Question
Explain the following reaction with the balanced equation.
Zinc sulphide is heated strongly in excess of air
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Solution
Zinc sulphide is heated strongly in excess of air to convert it to zinc oxide. This process is called roasting.
\[\ce{\underset{\text{Zinc sulphide}}{2ZnS_{(s)}} + 3O_{2(g)} -> \underset{\text{Zinc oxide}}{2ZnO_{(s)}} + \underset{\text{Sulphur dioxide}}{2SO_2↑}}\]
Notes
There is a printing mistake in the question.
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