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Chapter 22: Problem 81

Write a balanced equation for the reaction of each of the following compounds with water: (a) \(\mathrm{PCl}_{5}(s),\) (b) \(\mathrm{CO}_{2}(g)\) (c) \(\mathrm{K}_{2} \mathrm{O}_{2}(s)\) (d) \(\mathrm{Mg}_{3} \mathrm{P}_{2}(s)\) (e) \(\operatorname{LiAlH}_{4}(s)\) (f) \(\mathrm{Cl}_{2} \mathrm{O}(g)\) (g) \(\mathrm{NO}_{2}(g)\)

Short Answer

Expert verified
The balanced chemical equations for the given reactions are: (a) \( PCl_5(s) + 4H_2O(l) \rightarrow H_3PO_4(aq) + 5HCl(aq) \) (b) \( CO_2(g) + H_2O(l) \rightarrow H_2CO_3(aq) \) (c) \( K_2O_2(s) + 2H_2O(l) \rightarrow 2KOH(aq) + O_2(g) \) (d) \( Mg_3P_2(s) + 6H_2O(l) \rightarrow 3Mg(OH)_2(s) + 2PH_3(g) \) (e) \( LiAlH_4(s) + 4H_2O(l) \rightarrow LiOH(aq) + Al(OH)_3(s) + 4H_2(g) \) (f) \( Cl_2O(g) + H_2O(l) \rightarrow 2HCl(aq) + HOCl(aq) \) (g) \( 3NO_2(g) + H_2O(l) \rightarrow 2HNO_3(aq) + HNO_2(aq) \)

Step by step solution

01

(Reaction of PCl5 with water)

In this case, phosphorus pentachloride (PCl5) reacts with water (H2O) to produce phosphoric acid (H3PO4) and hydrochloric acid (HCl). The balanced equation for this reaction is: \( PCl_5(s) + 4H_2O(l) \rightarrow H_3PO_4(aq) + 5HCl(aq) \)
02

(Reaction of CO2 with water)

Carbon dioxide (CO2) reacts with water (H2O) to form carbonic acid (H2CO3). The balanced equation for this reaction is: \( \mathrm{CO}_{2}(g) + \mathrm{H}_{2}\mathrm{O}(l) \rightarrow \mathrm{H}_{2}\mathrm{CO}_{3}(aq) \)
03

(Reaction of K2O2 with water)

Potassium peroxide (K2O2) reacts with water (H2O) to produce potassium hydroxide (KOH) and oxygen gas (O2). The balanced equation for this reaction is: \( \mathrm{K}_{2} \mathrm{O}_{2}(s) + 2\mathrm{H}_{2}\mathrm{O}(l) \rightarrow 2\mathrm{KOH}(aq) + \mathrm{O}_{2}(g) \)
04

(Reaction of Mg3P2 with water)

Magnesium phosphide (Mg3P2) reacts with water (H2O) to produce magnesium hydroxide (Mg(OH)2) and phosphine gas (PH3). The balanced equation for this reaction is: \( \mathrm{Mg}_{3} \mathrm{P}_{2}(s) + 6\mathrm{H}_{2}\mathrm{O}(l) \rightarrow 3\mathrm{Mg(OH)}_{2}(s) + 2\mathrm{PH}_{3}(g) \)
05

(Reaction of LiAlH4 with water)

Lithium aluminum hydride (LiAlH4) reacts with water (H2O) to produce lithium hydroxide (LiOH), aluminum hydroxide (Al(OH)3), and hydrogen gas (H2). The balanced equation for this reaction is: \( \mathrm{LiAlH}_{4}(s) + 4\mathrm{H}_{2}\mathrm{O}(l) \rightarrow \mathrm{LiOH}(aq) + \mathrm{Al(OH)}_{3}(s) + 4\mathrm{H}_{2}(g) \)
06

(Reaction of Cl2O with water)

Dichlorine monoxide (Cl2O) reacts with water (H2O) to produce hydrochloric acid (HCl) and hypochlorous acid (HOCl). The balanced equation for this reaction is: \( \mathrm{Cl}_{2} \mathrm{O}(g) + \mathrm{H}_{2}\mathrm{O}(l) \rightarrow 2\mathrm{HCl}(aq) + \mathrm{HOCl}(aq) \)
07

(Reaction of NO2 with water)

Nitrogen dioxide (NO2) reacts with water (H2O) to produce nitric acid (HNO3) and nitrous acid (HNO2). The balanced equation for this reaction is: \( 3\mathrm{NO}_{2}(g) + \mathrm{H}_{2}\mathrm{O}(l) \rightarrow 2\mathrm{HNO}_{3}(aq) + \mathrm{HNO}_{2}(aq) \)

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Most popular questions from this chapter

Account for the following observations: (a) Phosphorus forms a pentachloride, but nitrogen does not. (b) \(\mathrm{H}_{3} \mathrm{PO}_{2}\) is a monoprotic acid. (c) Phosphonium salts, such as \(\mathrm{PH}_{4} \mathrm{Cl}\), can be formed under anhydrous conditions, but they cannot be made in aqueous solution. (d) White phosphorus is more reactive than red phosphorus.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium azide, (b) ammonium ion, (c) nitrous acid, \((\mathbf{d})\) magnesium nitride, \((\mathbf{e})\) diazene, \((\mathbf{f})\) sodium nitrate, (g) nitrogen trifluoride, (h) nitric acid.

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\) (c) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\).

Account for the following observations: (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) is a diprotic acid. (b) Nitric acid is a strong acid, whereas phos- (c) Phosphate rock is ineffective as a phoric acid is weak. phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does. (e) Solutions of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) are quite basic.
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