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Chapter 22: Problem 61

Use information from this chapter and previous chapters to write chemical equations to represent the following: (a) equilibrium between nitrogen dioxide and dinitrogen tetroxide in the gaseous state (b) the reduction of nitrous acid by \(\mathrm{N}_{2} \mathrm{H}_{5}^{+}\) forming hydrazoic acid, followed by the reduction of additional nitrous acid by the hydrazoic acid, yielding nitrogen and dinitrogen monoxide (c) the neutralization of \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})\) to the second equivalence point by \(\mathrm{NH}_{3}(\mathrm{aq})\).

Short Answer

Expert verified
The chemical reactions are: (a) \(2NO2(g) \leftrightarrows N2O4(g)\), (b) \(2HNO2(aq) + N2H5+(aq) \rightarrow 2HN3(aq) + H2O(l)\), and \(HN3(aq) + HNO2(aq) \rightarrow N2(g) + N2O(g) + H2O(l)\), (c) \(H3PO4(aq) + 2NH3(aq) \rightarrow (NH4)2HPO4(aq)\)

Step by step solution

01

Nitrogen Equilibrium

To represent the equilibrium between nitrogen dioxide (NO2) and dinitrogen tetroxide (N2O4), the reactants and products should be written on separate sides of the equation, with an equilibrium arrow in between. Both compounds are in the gaseous state: \(2NO2(g) \leftrightarrows N2O4(g)\)
02

Nitrous Acid Reduction

The reduction of nitrous acid (HNO2) by N2H5+ forms hydrazoic acid (HN3). Another HNO2 then reacts with the HN3 to yield nitrogen (N2) and dinitrogen monoxide(N2O): \(2HNO2(aq) + N2H5+(aq) \rightarrow 2HN3(aq) + H2O(l)\), \(HN3(aq) + HNO2(aq) \rightarrow N2(g) + N2O(g) + H2O(l)\)
03

PHosphoric Acid Neutralization

The neutralization of phosphoric acid (H3PO4) to the second equivalence point by ammonia (NH3). This means that two equivalence of ammonia react with one of phosphoric acid: \(H3PO4(aq) + 2NH3(aq) \rightarrow (NH4)2HPO4(aq)\)

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Most popular questions from this chapter

A 25.0 L sample of a natural gas, measured at \(25^{\circ} \mathrm{C}\). and 740.0 Torr, is bubbled through \(\mathrm{Pb}^{2+}(\mathrm{aq}),\) yielding \(0.535 \mathrm{g}\) of \(\mathrm{PbS}(\mathrm{s}) .\) What mass of sulfur can be recovered per cubic meter of this natural gas?

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) \(\mathrm{I}_{3}^{-}(\mathrm{aq})\).

Chemists have successfully synthesized the ionic compound \(\left[\mathrm{N}_{5}\right]\left[\mathrm{SbF}_{6}\right],\) which consists of \(\mathrm{N}_{5}^{+}\) and \(\mathrm{SbF}_{6}^{-}\) ions. Draw Lewis structures for these ions and assign formal charges to the atoms in your structures. Describe the structures of these ions. [Hint: The skeleton structure for \(\mathrm{N}_{5}^{+}\) is \(\mathrm{N}-\mathrm{N}-\mathrm{N}-\mathrm{N}-\mathrm{N}\) and several resonance structures can be drawn.].

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{S}_{2} \mathrm{Br}_{2}\) (b) \(\mathrm{SCl}_{2}\) (c) \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}_{4} \mathrm{O}_{6}\).

Joseph Priestley, a British chemist, was credited with the discovering oxygen in \(1774 .\) In his experiments, he generated oxygen gas by heating \(\mathrm{HgO}(\mathrm{s}) .\) The other product of the decomposition reaction is \(\mathrm{Hg}(1) .\) What volume of wet \(\mathrm{O}_{2}(\mathrm{g})\) is obtained from the decomposition of \(1.0 \mathrm{g} \mathrm{HgO}(\mathrm{s}),\) if the gas is collected over water at \(25^{\circ} \mathrm{C}\) and a barometric pressure of \(756 \mathrm{mmHg} ?\) The vapor pressure of water is \(23.76 \mathrm{mmHg}\) at \(25^{\circ} \mathrm{C}\).
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