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Chapter 8: Problem 33

Complete and balance the equation for the decomposition of each of the following. $$ \begin{array}{ll}{\text { a. } \mathrm{HgO} \rightarrow} & {\text { c. AgCl } \rightarrow} \\ {\text { b. } \mathrm{H}_{2} \mathrm{O} \longrightarrow} & {\text { d. } \mathrm{KOH} \longrightarrow}\end{array} $$

Short Answer

Expert verified
The balanced equations for the decomposition are: a) \(2HgO \rightarrow 2Hg + O_2\), b) \(2H_2O \rightarrow 2H_2 + O_2\), c) \(2AgCl \rightarrow 2Ag + Cl_2\), and d) \(2KOH \rightarrow 2K + H_2O2\).

Step by step solution

01

Decomposition and Balancing of HgO

HgO decomposes into mercury and oxygen. So, the equation becomes: \(HgO \rightarrow Hg + O_2\). However, this equation is not balanced. To balance it, we need to put a 2 in front of Hg and HgO. This leads to the balanced equation: \(2HgO \rightarrow 2Hg + O_2\).
02

Decomposition and Balancing of H2O

H2O decomposes into hydrogen and oxygen. The equation becomes: \(H_2O \rightarrow H_2 + O_2\). But this is not balanced. To resolve this, we add a 2 in front of H2O and H2. The balanced equation is: \(2H_2O \rightarrow 2H_2 + O_2\).
03

Decomposition and Balancing of AgCl

AgCl decomposes into silver and chlorine. The equation becomes: \(AgCl \rightarrow Ag + Cl_2\). But this is not balanced. To resolve this, we add a 2 in front of Ag and AgCl. The balanced equation is: \(2AgCl \rightarrow 2Ag + Cl_2\).
04

Decomposition and Balancing of KOH

KOH decomposes into potassium and water. The equation becomes: \(KOH \rightarrow K + H_2O\). But this is not balanced. To resolve this, we add a 2 in front of H2O and H2. The balanced equation is: \(2KOH \rightarrow 2K + H_2O2\).

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Most popular questions from this chapter

Write a balanced equation for each of the following: $$\begin{array}{c}{\text { a. copper(II) sulfate }+\text { ammonium sulfide } \rightarrow} \\ {\text { copper(II) sulfide + ammonium sulfate }} \\ {\text { b. nitric acid + barium hydroxide } \rightarrow} \\ {\text { water + barium nitrate }}\end{array}$$ $$ \begin{array}{c}{\text { c. barium chloride + phosphoric acid } \rightarrow} \\\ {\text { barium phosphate + hydrochloric acid }}\end{array} $$

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