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Chapter 4: Problem 9

Write balanced equations to represent: (a) the decomposition, by heating, of solid ammonium nitrate to produce dinitrogen monoxide gas (laughing gas) and water vapor (b) the reaction of aqueous sodium carbonate with hydrochloric acid to produce water, carbon dioxide gas, and aqueous sodium chloride (c) the reaction of methane \(\left(\mathrm{CH}_{4}\right),\) ammonia, and oxygen gases to form gaseous hydrogen cyanide (HCN) and water vapor

Short Answer

Expert verified
The balanced equations are: (a) \(\mathrm{NH}_4\mathrm{NO}_3 \rightarrow 2\mathrm{N}_2\mathrm{O} + 2\mathrm{H}_2\mathrm{O}\), (b) \(\mathrm{Na}_2\mathrm{CO}_3 + 2\mathrm{HCl} \rightarrow \mathrm{H}_2\mathrm{O} + \mathrm{CO}_2 + 2\mathrm{NaCl\), and (c) \(\mathrm{CH}_4 + 2\mathrm{NH}_3 + \frac{3}{2}\mathrm{O}_2 \rightarrow \mathrm{HCN} + 6\mathrm{H}_2\mathrm{O}\)

Step by step solution

01

Decomposition of solid ammonium nitrate by heating

The given decomposition reaction of solid ammonium nitrate is represented as follows: \[ \mathrm{NH}_4\mathrm{NO}_3 \rightarrow \mathrm{N}_2\mathrm{O} + \mathrm{H}_2\mathrm{O} \] Counting the atoms on each side of the equation shows this is unbalanced. Adding coefficients to the reactants and products to balance the atoms and energy give us: \[ \mathrm{NH}_4\mathrm{NO}_3 \rightarrow 2\mathrm{N}_2\mathrm{O} + 2\mathrm{H}_2\mathrm{O}\]
02

Reaction of aqueous sodium carbonate with hydrochloric acid

The given reaction of aqueous sodium carbonate with hydrochloric acid can be written as: \[ \mathrm{Na}_2\mathrm{CO}_3 + \mathrm{HCl} \rightarrow \mathrm{H}_2\mathrm{O} + \mathrm{CO}_2 + \mathrm{NaCl}\] This equation is unbalanced. After balancing it, the following equation is achieved: \[ \mathrm{Na}_2\mathrm{CO}_3 + 2\mathrm{HCl} \rightarrow \mathrm{H}_2\mathrm{O} + \mathrm{CO}_2 + 2\mathrm{NaCl}\]
03

Reaction of methane, ammonia, and oxygen gases

The given reaction of methane, ammonia, and oxygen gases can be represented as follows: \[ \mathrm{CH}_4 + \mathrm{NH}_3 + \mathrm{O}_2 \rightarrow \mathrm{HCN} + \mathrm{H}_2\mathrm{O}\] This equation is unbalanced. After balancing it, the following balanced chemical equation can be written down: \[ \mathrm{CH}_4 + 2\mathrm{NH}_3 + \frac{3}{2}\mathrm{O}_2 \rightarrow \mathrm{HCN} + 6\mathrm{H}_2\mathrm{O} \]

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Most popular questions from this chapter

Chalkboard chalk is made from calcium carbonate and calcium sulfate, with minor impurities such as \(\mathrm{SiO}_{2} .\) Only the \(\mathrm{CaCO}_{3}\) reacts with dilute \(\mathrm{HCl}(\mathrm{aq})\) What is the mass percent \(\mathrm{CaCO}_{3}\) in a piece of chalk if a 3.28 -g sample yields \(0.981 \mathrm{g} \mathrm{CO}_{2}(\mathrm{g}) ?\) $$\begin{aligned} \mathrm{CaCO}_{3}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) & \longrightarrow \mathrm{CaCl}_{2}(\mathrm{aq}) +\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g}) \end{aligned}$$

When the equation below is balanced, the correct set of stoichiometric coefficients is (a) \(1,6 \longrightarrow 1,3,4;\) (b) \(1,4 \longrightarrow 1,2,2 ;\) (c) \(2,6 \longrightarrow 2,3,2;\) (d) \(3,8 \longrightarrow 3,4,2\) \(\begin{aligned} ? \mathrm{Cu}(\mathrm{s})+? \mathrm{HNO}_{3}(\mathrm{aq}) & \longrightarrow ? \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+? \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+? \mathrm{NO}(\mathrm{g}) \end{aligned}\)

In your own words, define or explain these terms or symbols. (a) \(\stackrel{\Delta}{\longrightarrow}\) (b) (aq) (c) stoichiometric coefficient (d) overall equation

How many grams of commercial acetic acid (97\% \(\mathrm{CH}_{3} \mathrm{COOH}\) by mass) must be allowed to react with an excess of \(\mathrm{PCl}_{3}\) to produce \(75 \mathrm{g}\) of acetyl chloride \(\left(\mathrm{CH}_{3} \mathrm{COCl}\right),\) if the reaction has a \(78.2 \%\) yield? $$\begin{aligned} \mathrm{CH}_{3} \mathrm{COOH}+\mathrm{PCl}_{3} & \longrightarrow \mathrm{CH}_{3} \mathrm{COCl}+ \mathrm{H}_{3} \mathrm{PO}_{3}(\text { not balanced }) \end{aligned}$$

Lead nitrate and potassium iodide react in aqueous solution to form a yellow precipitate of lead iodide. In one series of experiments, the masses of the two reactants were varied, but the total mass of the two was held constant at \(5.000 \mathrm{g}\). The lead iodide formed was filtered from solution, washed, dried, and weighed. The table gives data for a series of reactions. $$\begin{array}{lll} \hline & \text { Mass of Lead } & \text { Mass of Lead } \\ \text { Experiment } & \text { Nitrate, } g & \text { lodide, } g \\ \hline 1 & 0.500 & 0.692 \\ 2 & 1.000 & 1.388 \\ 3 & 1.500 & 2.093 \\ 4 & 3.000 & 2.778 \\ 5 & 4.000 & 1.391 \\ \hline \end{array}$$ (a) Plot the data in a graph of mass of lead iodide versus mass of lead nitrate, and draw the appropriate curve(s) connecting the data points. What is the maximum mass of precipitate that can be obtained? (b) Explain why the maximum mass of precipitate is obtained when the reactants are in their stoichiometric proportions. What are these stoichiometric proportions expressed as a mass ratio, and as a mole ratio? (c) Show how the stoichiometric proportions determined in part (b) are related to the balanced equation for the reaction.
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