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Chapter 22: Problem 25

Each of the following compounds decomposes to produce \(\mathrm{O}_{2}(\mathrm{g})\) when heated: \((\mathrm{a}) \mathrm{HgO}(\mathrm{s}) ;\) (b) \(\mathrm{KClO}_{4}(\mathrm{s})\) Write plausible equations for these reactions.

Short Answer

Expert verified
The balanced equations for the decomposition of HgO and KClO4 are: 2 HgO(s) → 2 Hg(l) + O2(g) and KClO4(s) → KCl(s) + 2 O2(g), respectively.

Step by step solution

01

Write Unbalanced Decomposition Reaction for HgO

In the decomposition of mercury(II) oxide (HgO), mercury and oxygen gas are formed. The reaction can be represented as: HgO(s) → Hg(l) + O2(g). But this is not balanced yet.
02

Balancing the Decomposition Reaction for HgO

The rule for balancing chemical equations is that the number of atoms for each element should be the same on both sides of the equation. There are 2 oxygen atoms on the right side while there is only 1 on the left side in our equation. To balance this, place a 2 in front of HgO, and 1 in front of Hg, which gives us the balanced equation is: 2 HgO(s) → 2 Hg(l) + O2(g)
03

Write Unbalanced Decomposition Reaction for KClO4

In the decomposition of potassium perchlorate (KClO4), potassium chloride and oxygen gas are formed. The reaction can be represented as: KClO4(s) → KCl(s) + O2(g). But this equation is not balanced yet.
04

Balancing the Decomposition Reaction for KClO4

Again, apply the rule that the number of atoms for each element in a chemical equation must be the same on both sides. In our equation, there are 4 oxygen atoms on the left side, but only 2 on the right side. To balance this, put a 2 in front of O2. This gives us our final balanced equation: KClO4(s) → KCl(s) + 2 O2(g).

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Most popular questions from this chapter

Each of the following compounds produces \(\mathrm{O}_{2}(\mathrm{g})\) when strongly heated: (a) \(\mathrm{HgO}(\mathrm{s}) ;\) (b) \(\mathrm{KClO}_{4}(\mathrm{s})\) (c) \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) ;\) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) .\) Write a plausible equation for the reaction that occurs in each instance.

Draw Lewis structures for \(\mathrm{O}_{3}\) and \(\mathrm{SO}_{2}\). In what ways are the structures similar? In what ways do they differ?

Give an appropriate formula for each of the following compounds: (a) calcium sulfate dihydrate; (b) hydrosulfuric acid; (c) sodium hydrogen sulfate; (d) disulfuric acid.

Draw plausible Lewis structures for (a) dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\) (b) nitryl chloride, \(\mathrm{ClNO}_{2}\) (Central atom is \(\mathrm{N}\) ) (c) phosphorous acid, a diprotic acid with the empirical formula \(\mathrm{H}_{3} \mathrm{PO}_{3}\).

Make a general prediction about which of the halogen elements, \(\mathrm{F}_{2}, \mathrm{Cl}_{2}, \mathrm{Br}_{2},\) or \(\mathrm{I}_{2},\) displaces other halogens from a solution of halide ions. Which of the halogens is able to displace \(\mathrm{O}_{2}(\mathrm{g})\) from water? Which is able to displace \(\mathrm{H}_{2}(\mathrm{g})\) from water?
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