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Chapter 7: Problem 66

Write balanced equations for the following reactions: (a) sulfur dioxide with water, (b) lithium oxide in water, \((\mathbf{c})\) zinc oxide with dilute hydrochloric acid, \((\mathbf{d})\) arsenic trioxide with aqueous potassium hydroxide.

Short Answer

Expert verified
(a) \( \text{SO}_2 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_3 \); (b) \( \text{Li}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{LiOH} \); (c) \( \text{ZnO} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \); (d) \( \text{As}_2\text{O}_3 + 6\text{KOH} \rightarrow 2\text{K}_3\text{AsO}_3 + 3\text{H}_2\text{O} \).

Step by step solution

01

Understanding Reaction (a)

Sulfur dioxide reacts with water to form sulfurous acid. The equation is initially: \( \text{SO}_2 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_3 \). This equation is already balanced because there are equal numbers of each type of atom on both sides.
02

Understanding Reaction (b)

Lithium oxide reacts with water to form lithium hydroxide. The unbalanced equation is \( \text{Li}_2\text{O} + \text{H}_2\text{O} \rightarrow \text{LiOH} \). To balance it, ensure there are two lithium hydroxides, giving: \( \text{Li}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{LiOH} \).
03

Understanding Reaction (c)

Zinc oxide reacts with dilute hydrochloric acid (HCl) to form zinc chloride and water. The unbalanced equation is \( \text{ZnO} + \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \). Balancing it, add a coefficient of 2 to HCl: \( \text{ZnO} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \).
04

Understanding Reaction (d)

Arsenic trioxide reacts with aqueous potassium hydroxide to form potassium arsenite and water. The unbalanced equation is \( \text{As}_2\text{O}_3 + \text{KOH} \rightarrow \text{K}_3\text{AsO}_3 + \text{H}_2\text{O} \). Balancing yields: \( \text{As}_2\text{O}_3 + 6\text{KOH} \rightarrow 2\text{K}_3\text{AsO}_3 + 3\text{H}_2\text{O} \).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Balancing Equations
Balancing chemical equations is a fundamental skill in chemistry. It ensures that the number of atoms for each element is equal on both sides of a reaction, adhering to the Law of Conservation of Mass. Each molecule or compound is represented by its chemical formula, and we adjust the coefficients (the numbers before each compound) to make the equation balanced.

For example, let's consider the reaction between zinc oxide and hydrochloric acid:
  • Initial unbalanced equation: \( \text{ZnO} + \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \)
  • Balance chlorine by adding a coefficient of 2 in front of HCl, resulting in: \( \text{ZnO} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \)
This adjustment ensures that there are two chlorine atoms on each side, as well as all other elements balanced. This approach is used in all reactions, regardless of complexity.
Sulfur Compounds
Sulfur compounds, especially in the form of oxides, play a major role in various chemical processes. Sulfur dioxide (\( \text{SO}_2 \)) is a common compound where sulfur is combined with oxygen.

When sulfur dioxide reacts with water, it produces sulfurous acid:
  • Chemical reaction: \( \text{SO}_2 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_3 \)
  • This balanced equation shows that sulfur dioxide combines equally with water, forming sulfurous acid with no leftover reactants.
Understanding reactions involving sulfur compounds is key for topics like acid rain and industrial processes.
Oxides
Oxides are chemical compounds that consist of at least one oxygen atom and one other element. They can be found everywhere, from the Earth's crust to our everyday life.
Types of Oxides:
  • Metal Oxides: Often form bases, such as lithium oxide (\( \text{Li}_2\text{O} \)) reacting with water to form lithium hydroxide (an alkaline compound).
  • Non-metal Oxides: Typically form acids, like sulfur dioxide forming sulfurous acid.
Oxides interact dynamically in nature and human-made processes. Balancing reactions involving oxides is a common task in chemistry.
Hydrochloric Acid
Hydrochloric acid (HCl) is a strong acid commonly used in laboratories and industrial settings. It reacts with various compounds to form salts and water. It's crucial in reactions involving metals and oxides, such as the reaction with zinc oxide:
  • Reaction: \( \text{ZnO} + \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \)
  • Balanced form: \( \text{ZnO} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2\text{O} \)
Understanding how and why HCl interacts with different substances deepens our insight into both natural and industrial chemical processes.

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Most popular questions from this chapter

Identify a +2 cation that has the following ground state electron configurations: (a) \([\mathrm{Ne}]\) (b) \([\mathrm{Ar}] 3 d^{9}\) (c) \([\mathrm{Xe}] 4 \mathrm{f}^{14} 5 d^{10} 6 s^{2}\).

Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen, (b) the second ionization energy of ox ' ygen, and \((\mathbf{c})\) the electron affinity of oxygen? (i) \(\mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g)\) (ii) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{+}(g)+\mathrm{e}^{-}\) (iii) \(\mathrm{O}(g)+2 \mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g)\) (iv) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{2+}(g)+2 \mathrm{e}^{-}\) \((\mathbf{v}) \mathrm{O}^{+}(g) \longrightarrow \mathrm{O}^{2+}(g)+\mathrm{e}^{-}\)

Write equations that show the process for (a) the first two ionization energies of zinc and (b) the fourth ionization energy of calcium.

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\). When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for the reaction of the white substance with water.

Which neutral atom is isoelectronic with each of the following ions? \(\mathrm{H}^{-}, \mathrm{Ca}^{2+}, \mathrm{In}^{3+}, \mathrm{Ge}^{2+}\)
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