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Chapter 22: Problem 47

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid.(c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.

Short Answer

Expert verified
(a) \( SO_2 (g) + H_2O (l) \rightarrow H_2SO_3 (aq) \) (b) \( ZnS (s) + 2 HCl (aq) \rightarrow ZnCl_2 (aq) + H_2S (g) \) (c) \( S (s) + SO_3^{2-} (aq) \rightarrow S_2O_3^{2-} (aq) \) (d) \( SO_3 (g) + H_2SO_4 (aq) \rightarrow H_2S_2O_7 (aq) \)

Step by step solution

01

(a) Sulfur dioxide reacts with water.

First, we need to write the general equation for this reaction: SO₂ (g) + H₂O (l) → H₂SO₃ (aq) Now, we can see that the number of atoms for each element matches on both sides, as we have 1 sulfur atom, 2 hydrogen atoms, and 3 oxygen atoms on both the reactant and product sides. This means the equation is already balanced: SO₂ (g) + H₂O (l) → H₂SO₃ (aq)
02

(b) Solid zinc sulfide reacts with hydrochloric acid.

First, let's write the general equation for this reaction: ZnS (s) + HCl (aq) → ZnCl₂ (aq) + H₂S (g) Now, we need to balance the equation. To do this, we see that there are 2 Cl atoms on the product side but only 1 on the reactant side, so we need to add a coefficient of 2 in front of the HCl: ZnS (s) + 2 HCl (aq) → ZnCl₂ (aq) + H₂S (g) Now the equation is balanced, with 1 Zn, 1 S, and 2 H and Cl atoms on both sides.
03

(c) Elemental sulfur reacts with sulfite ion to form thiosulfate.

First, let's write the general equation for this reaction: S (s) + SO₃²⁻ (aq) → S₂O₃²⁻ (aq) Now, we need to balance the equation. The equation is already balanced since there are 1 sulfur atom and 3 oxygen atoms on both sides of the equation.
04

(d) Sulfur trioxide is dissolved in sulfuric acid.

First, let's write the general equation for this reaction: SO₃ (g) + H₂SO₄ (aq) → H₂S₂O₇ (aq) Now, we need to balance the equation. The equation is already balanced since there are 2 sulfur atoms, 2 hydrogen atoms, and 7 oxygen atoms on both sides.

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Most popular questions from this chapter

Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until \(1965 .\) The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?

Complete and balance the following equations: $$\begin{array}{l}{\text { (a) } \operatorname{NaH}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (b) } \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow} \\\ {\text { (c) } \mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow}\end{array}$$ $$\begin{array}{l}{\text {{(d)} ) ~ } \mathrm{Na}(l)+\mathrm{H}_{2}(g) \longrightarrow} \\ {\text { (e) } \mathrm{PbO}(s)+\mathrm{H}_{2}(g) \longrightarrow}\end{array}$$

Select the more acidic member of each of the following pairs: (a) \(\mathrm{Mn}_{2} \mathrm{O}_{7}\) and \(\mathrm{MnO}_{2},(\mathbf{b}) \mathrm{SnO}\) and \(\mathrm{SnO}_{2},(\mathbf{c}) \mathrm{SO}_{2}\) and \(\mathrm{SO}_{3},(\mathbf{d}) \mathrm{SiO}_{2}\) and \(\mathrm{SO}_{2},(\mathbf{e}) \mathrm{Ga}_{2} \mathrm{O}_{3}\) and \(\mathrm{In}_{2} \mathrm{O}_{3},(\mathbf{f}) \mathrm{SO}_{2}\) and \(\mathrm{SeO}_{2} .\)

Complete and balance the following equations: $$\begin{array}{l}{\text { (a) } \mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (b) } \mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow} \\\ {\text { (c) } \mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow}\end{array}$$ $$ \begin{array}{l}{\text {(d) } \mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (e) } \mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (f) } \mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow}\end{array} $$

Hydrazine has been employed as a reducing agent for metals. Using standard reduction potentials, predict whether the following metals can be reduced to the metallic state by hydrazine under standard conditions in acidic solution: (a) \(\mathrm{Fe}^{2+},(\mathbf{b}) \mathrm{Sn}^{2+},(\mathbf{c}) \mathrm{Cu}^{2+},(\mathbf{d}) \mathrm{Ag}^{+},(\mathbf{e}) \mathrm{Cr}^{3+},(\mathbf{f}) \mathrm{Co}^{3+}\)
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