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Chapter 22: Problem 129

Complete and balance equations for these reactions. (a) \(\operatorname{LiH}(s)+H_{2} O(1) \longrightarrow\) (b) \(\mathrm{C}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow}\) (c) \(\mathrm{NO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\)

Short Answer

Expert verified
The three balanced equations are: (a) \(\operatorname{LiH}(s)+H_{2} O(l) \longrightarrow LiOH(aq) + H_{2}(g)\), (b) \(\mathrm{C}(s) + H_{2} O(g) \stackrel{\Delta}{\longrightarrow} CO(g) + H_{2}(g)\), (c) \(\mathrm{NO}_{2}(g) + H_{2} O(l) \longrightarrow HNO_{3}(aq) + NO(g)\)

Step by step solution

01

Balancing Equation (a)

Equation (a) is as follows \(\operatorname{LiH}(s)+H_{2} O(l) \longrightarrow\). You need to make sure the number and type of atoms on both sides of the equation are equal. The balanced equation is \(\operatorname{LiH}(s)+H_{2} O(l) \longrightarrow LiOH(aq) + H_{2}(g)\)
02

Balancing Equation (b)

Equation (b) is \( \mathrm{C}(s) + H_{2} O(g) \stackrel{\Delta}{\longrightarrow}\). Again, you need to balance the elements on both sides of the equation. The balanced equation would be \(\mathrm{C}(s) + H_{2} O(g) \stackrel{\Delta}{\longrightarrow} CO(g) + H_{2}(g)\)
03

Balancing Equation (c)

Equation (c) is \(\mathrm{NO}_{2}(g) + H_{2} O(l) \longrightarrow\). Balancing the equation would give: \(\mathrm{NO}_{2}(g) + H_{2} O(l) \longrightarrow HNO_{3}(aq) + NO(g)\)

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Most popular questions from this chapter

To displace \(\mathrm{Br}_{2}\) from an aqueous solution of \(\mathrm{Br}^{-}\) add \((\mathrm{a}) \mathrm{I}_{2}(\mathrm{aq}) ;\) (b) \(\mathrm{Cl}_{2}(\mathrm{aq}) ;\) (c) \(\mathrm{H}_{2}(\mathrm{g}) ;\) (d) \(\mathrm{Cl}^{-}(\mathrm{aq})\) (e) \(\mathrm{I}_{3}^{-}(\mathrm{aq})\).

The heavier halogens (Cl, Br, and I) form compounds in which the central halogen atom, \(X\), is bonded directly to oxygen and to fluorine. Several examples are known, including those with formulas of the type \(\mathrm{FXO}_{2}, \mathrm{FXO}_{3, \text { and } \mathrm{F}_{3} \mathrm{XO} . \text { The structures of these }}\) molecules are all consistent with the VSEPR model. Draw Lewis structures and predict the geometries of (a) chloryl fluoride, \(\mathrm{FClO}_{2}\); (b) perchloryl fluoride, \(\mathrm{FClO}_{3} ;(\mathrm{c}) \mathrm{F}_{3} \mathrm{ClO}\).

One reaction of a chlorofluorocarbon implicated in the destruction of stratospheric ozone is \(\mathrm{CFCl}_{3}+h v \longrightarrow \mathrm{CFCl}_{2}+\mathrm{Cl}\) (a) What is the energy of the photons ( \(h v\) ) required to bring about this reaction, expressed in kilojoules per mole? (b) What is the frequency and wavelength of the light necessary to produce the reaction? In what portion of the electromagnetic spectrum is this light found?

Each of the following compounds produces \(\mathrm{O}_{2}(\mathrm{g})\) when strongly heated: (a) \(\mathrm{HgO}(\mathrm{s}) ;\) (b) \(\mathrm{KClO}_{4}(\mathrm{s})\) (c) \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) ;\) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) .\) Write a plausible equation for the reaction that occurs in each instance.

The following bond energies are given for \(298 \mathrm{K}: \mathrm{O}_{2}\) \(498 ; \mathrm{N}_{2}, 946 ; \mathrm{F}_{2}, 159 ; \mathrm{Cl}_{2}, 243 ;\) ClF, \(251 ; \mathrm{OF}\left(\text { in } \mathrm{OF}_{2}\right)\) \(213 ; \mathrm{ClO}\left(\operatorname{in} \mathrm{Cl}_{2} \mathrm{O}\right), 205 ;\) and \(\mathrm{NF}\left(\mathrm{in} \mathrm{NF}_{3}\right), 280 \mathrm{kJmol}^{-14}\) Calculate \(\Delta H_{f}\) at \(298 \mathrm{K}\) for \(1 \mathrm{mol}\) of \((\mathrm{a}) \mathrm{ClF}(\mathrm{g})\) (b) \(\mathrm{OF}_{2}(\mathrm{g}) ;(\mathrm{c}) \mathrm{Cl}_{2} \mathrm{O}(\mathrm{g}) ;(\mathrm{d}) \mathrm{NF}_{3}(\mathrm{g})\).
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