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Chapter 8: Problem 103

Mineral compounds containing sulfur are converted to oxygen-containing compounds by a process known as roasting, which involves heating the mineral in the presence of oxygen. In addition to the mineral oxide, sulfur dioxide is also produced. Write the balanced chemical equation for the roasting of zinc sulfide, \(\mathrm{ZnS}\), to produce zinc oxide, \(\mathrm{ZnO}\), plus sulfur dioxide.

Short Answer

Expert verified
The balanced chemical equation for the roasting of zinc sulfide (ZnS) to produce zinc oxide (ZnO) and sulfur dioxide (SO2) is: 2 ZnS + O2 -> 2 ZnO + 2 SO2

Step by step solution

01

Write the unbalanced chemical equation

The reaction between zinc sulfide (ZnS) and oxygen (O2) produces zinc oxide (ZnO) and sulfur dioxide (SO2). The unbalanced equation for this reaction is: ZnS + O2 -> ZnO + SO2
02

Balance the chemical equation

In order to balance the equation, we must ensure that there are equal numbers of atoms of each element on both sides of the equation. We can see that there are an equal number of zinc atoms on both sides, so we only need to balance the sulfur and oxygen atoms. In the unbalanced equation, we have 1 sulfur atom on both sides of the equation and 2 oxygen atoms on the left side and 3 oxygen atoms on the right side. To balance it, we can multiply O2 by 1/2 and SO2 by 1 to get the following balanced equation: ZnS + 1/2 O2 -> ZnO + 1 SO2 Another way to avoid fractions in chemical equations is to double the coefficients of the entire reaction. So, the final balanced equation would be: 2 ZnS + O2 -> 2 ZnO + 2 SO2

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