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Chapter 22: Problem 40

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

Short Answer

Expert verified
(a) \(\mathrm{CaO}(s) + 2\mathrm{H_2O}(l) \longrightarrow \mathrm{Ca(OH)_2}(aq)\) (b) \(\mathrm{Al_2O_3}(s) + 6\mathrm{H^+}(aq) \longrightarrow 2\mathrm{Al^{3+}}(aq) + 3\mathrm{H_2O}(l)\) (c) \(\mathrm{Na_2O_2}(s) + 2\mathrm{H_2O}(l) \longrightarrow 2\mathrm{NaOH}(aq) + \mathrm{H_2O_2}(aq)\) (d) \(\mathrm{N_2O_3}(g) + \mathrm{H_2O}(l) \longrightarrow 2\mathrm{HNO_2}(aq)\) (e) \(\mathrm{KO_2}(s) + 2\mathrm{H_2O}(l) \longrightarrow 2\mathrm{KOH}(aq) + \mathrm{H_2O_2}(aq) + \mathrm{O_2}(g)\) (f) \(2\mathrm{NO}(g) + \mathrm{O_3}(g) \longrightarrow \mathrm{N_2O_5}(g)\)

Step by step solution

01

(a) Balancing the CaO and H2O equation

To balance this equation, first identify the number of atoms of each element on both sides of the equation. Ca and O are balanced, but there's 1 H atom on the left and 2 H atoms on the right. To balance the H atoms, add a coefficient of 2 in front of the H2O on the left side. The balanced equation is: \(\mathrm{CaO}(s) + 2\mathrm{H_2O}(l) \longrightarrow \mathrm{Ca(OH)_2}(aq)\)
02

(b) Balancing the Al2O3 and H+ equation

Balance the Al and O atoms. Add a coefficient of 6 in front of the H+ on the right side to balance the O atoms. Now there are 3 Al atoms on the left and 6 O atoms on both sides. Thus, the balanced equation is: \(\mathrm{Al_2O_3}(s) + 6\mathrm{H^+}(aq) \longrightarrow 2\mathrm{Al^{3+}}(aq) + 3\mathrm{H_2O}(l)\)
03

(c) Balancing the Na2O2 and H2O equation

Balance the Na, O, and H atoms. Add a coefficient of 2 in front of the H2O on the right side to balance the O atoms. Now there are 2 Na atoms on both sides and 2 H atoms on both sides. The balanced equation is: \(\mathrm{Na_2O_2}(s) + 2\mathrm{H_2O}(l) \longrightarrow 2\mathrm{NaOH}(aq) + \mathrm{H_2O_2}(aq)\)
04

(d) Balancing the N2O3 and H2O equation

Balance the N, O, and H atoms. Add a coefficient of 2 in front of the H2O on the right side to balance the N atoms. Now there are 2 N atoms and 5 O atoms on both sides. Thus, the balanced equation is: \(\mathrm{N_2O_3}(g) + \mathrm{H_2O}(l) \longrightarrow 2\mathrm{HNO_2}(aq)\)
05

(e) Balancing the KO2 and H2O equation

Balance the K, O, and H atoms. Add a coefficient of 2 in front of the H2O on the right side to balance the O atoms. Now there are 2 K atoms on both sides and 2 H atoms on both sides. The balanced equation is: \(\mathrm{KO_2}(s) + 2\mathrm{H_2O}(l) \longrightarrow 2\mathrm{KOH}(aq) + \mathrm{H_2O_2}(aq) + \mathrm{O_2}(g)\)
06

(f) Balancing the NO and O3 equation

Balance the N and O atoms. Add a coefficient of 2 in front of the NO on the left side to balance the N atoms. Now there are 2 N atoms and 5 O atoms on both sides. Thus, the balanced equation is: \(2\mathrm{NO}(g) + \mathrm{O_3}(g) \longrightarrow \mathrm{N_2O_5}(g)\)

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Most popular questions from this chapter

Give a reason why hydrogen might be placed along with the group lA elements of the periodic table.

What is the anhydride for each of the following acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{HClO}_{3}\) (c) \(\mathrm{HNO}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (e) \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the (a) \(\mathrm{NH}_{4}^{+},(\mathbf{b}) \mathrm{NO}_{2}^{-}\), nitrogen: (c) \(\mathrm{N}_{2} \mathrm{O},(\mathrm{d}) \mathrm{NO}_{2}\)

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

Explain each of the following observations: (a) At room temperature \(\mathrm{I}_{2}\) is a solid, \(\mathrm{Br}_{2}\) is a liquid, and \(\mathrm{Cl}_{2}\) and \(\mathrm{F}_{2}\) are both gases. (b) \(\mathrm{F}_{2}\) cannot be prepared by electrolytic oxidation of aqueous \(\mathrm{F}^{-}\) solutions. (c) The boiling point of \(\mathrm{HF}\) is much higher than those of the other hydrogen halides. (d) The halogens decrease in oxidizing power in the order \(\mathrm{F}_{2}>\mathrm{Cl}_{2}>\mathrm{Br}_{2}>\mathrm{I}_{2}\)
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