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Chapter 22: Problem 56

When heated, each of the following substances decomposes to the products indicated. Write balanced equations for these reactions. (a) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s})\) to \(\mathrm{N}_{2}(\mathrm{g}), \mathrm{O}_{2}(\mathrm{g}),\) and \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (b) \(\mathrm{NaNO}_{3}(\mathrm{s})\) to sodium nitrite and oxygen gas (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s})\) to lead(II) oxide, nitrogen dioxide, and oxygen.

Short Answer

Expert verified
Balanced equations are: (a) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})+2\mathrm{H}_{2}\mathrm{O}(\mathrm{g})\), (b) \(2\mathrm{NaNO}_{3}(\mathrm{s}) \rightarrow 2\mathrm{NaNO}_{2}(\mathrm{s}) + \mathrm{O}_{2}(\mathrm{g})\), and (c) \(2\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) \rightarrow 2 \mathrm{PbO}(\mathrm{s}) + 4 \mathrm{NO}_{2}(\mathrm{g}) + \mathrm{O}_{2}(\mathrm{g})\).

Step by step solution

01

Balancing equation for \(\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s})\)

The reaction can be written initially as: \[ \mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2}\mathrm{O}(\mathrm{g}) \] By counting each atom type both in the reactants and products, and by adding respective coefficients, it can be balanced as: \[ \mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})+2\mathrm{H}_{2}\mathrm{O}(\mathrm{g}) \]
02

Balancing equation for \(\mathrm{NaNO}_{3}(\mathrm{s})\)

The reaction can be written initially as: \[ \mathrm{NaNO}_{3}(\mathrm{s}) \rightarrow \mathrm{NaNO}_{2}(\mathrm{s}) + \mathrm{O}_{2}(\mathrm{g}) \] By counting each atom type both in the reactants and products, and by adding a coefficient, it can be balanced as: \[ 2\mathrm{NaNO}_{3}(\mathrm{s}) \rightarrow 2\mathrm{NaNO}_{2}(\mathrm{s}) + \mathrm{O}_{2}(\mathrm{g}) \]
03

Balancing equation for \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s})\)

The reaction can initially be written as: \[ \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) \rightarrow \mathrm{PbO}(\mathrm{s}) + \mathrm{NO}_{2}(\mathrm{g}) + \mathrm{O}_{2}(\mathrm{g}) \] By counting each atom type both in the reactants and products, and by adding respective coefficients, it can be balanced as: \[ 2\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) \rightarrow 2 \mathrm{PbO}(\mathrm{s}) + 4 \mathrm{NO}_{2}(\mathrm{g}) + \mathrm{O}_{2}(\mathrm{g}) \]

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Most popular questions from this chapter

The structures of the \(\mathrm{NH}_{3}\) and \(\mathrm{NF}_{3}\) molecules are similar, yet the dipole moment for the \(\mathrm{NH}_{3}\) molecule is rather large (1.47 debye) and that of the NF \(_{3}\) molecule is rather small (0.24 debye). Provide an explanation for this difference in the dipole moments.

The best reducing agent of the following substances is (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{O}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) (d) \(\mathrm{NaF}\); (e) \(\mathrm{H}_{2} \mathrm{O}\).

Use Lewis structures and other information to explain the observation that (a) the oxygen-to-oxygen bond lengths in \(\mathrm{O}_{2}, \mathrm{O}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}_{2}\) are \(121,128,\) and \(148 \mathrm{pm},\) respectively. (b) the oxygen-to-oxygen bond length of \(\mathrm{O}_{2}\) is \(121 \mathrm{pm}\) and for \(\mathrm{O}_{2}^{+}\) is \(112 \mathrm{pm}\). Why is the bond length for \(\mathrm{O}_{2}^{+}\) so much shorter than for \(\mathrm{O}_{2} ?\)

The text mentions that ammonium perchlorate is an explosion hazard. Assuming that \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) is the sole reactant in the explosion, write a plausible equation(s) to represent the reaction that occurs.

Write balanced equations for the following important commercial reactions involving nitrogen and its compounds. (a) the principal artificial method of fixing atmospheric \(\mathrm{N}_{2}\) (b) oxidation of ammonia to \(\mathrm{NO}\) (c) preparation of nitric acid from \(\mathrm{NO}\).
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