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Chapter 22: Problem 128

Give a practical laboratory method that you might use to produce small quantities of the following gases and comment on any difficulties that might arise: (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{NO} ;\) (c) \(\mathrm{H}_{2} ;\) (d) \(\mathrm{NH}_{3} ;\) (e) \(\mathrm{CO}_{2}\).

Short Answer

Expert verified
The gases are produced in the following ways: \(O_2\) through decomposition of \(H_2O_2\), \(NO\) by the reduction of concentrared \(HNO_3\) by copper, \(H_2\) by the reaction of zinc with \(H_2SO_4\), \(NH_3\) by the reaction of \(NH_4Cl\) with \(NaOH\) and \(CO_2\) by the reaction of \(CaCO_3\) with \(HCl\). Safety measures should be adhered to due to the potentially harmful and corrosive substances used.

Step by step solution

01

Production of Oxygen (\(O_2\))

Oxygen can be generated in a lab by the decomposition of hydrogen peroxide (\(H_2O_2\)). This is usually done by adding a catalyst like manganese dioxide (\(MnO_2\)) to speed up the reaction. The reaction is: \(2H_2O_2 \rightarrow 2H_2O + O_2\). The difficulty in this method is handling the manganese dioxide catalyst as it is harmful when inhaled or swallowed.
02

Production of Nitric Oxide (\(NO\))

Nitric oxide can be produced by the reduction of concentrated nitric acid (\(HNO_3\)) by copper. The reaction is: \(3Cu + 8HNO_3 \rightarrow 3Cu(NO_3)_2 + 2NO + 4H_2O\). The difficulty in this method could be handling of the nitric acid as it is quite corrosive.
03

Production of Hydrogen (\(H_2\))

Hydrogen can be produced in the lab by the reaction between zinc and sulfuric acid (\(H_2SO_4\)). The reaction is: \(Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2\). The difficulty could be the handling of sulfuric acid which is corrosive and can cause burns.
04

Production of Ammonia (\(NH_3\))

In a lab, ammonia can be prepared by the reaction of a salt like ammonium chloride (\(NH_4Cl\)) with a strong alkali like sodium hydroxide (\(NaOH\)). The reaction is: \(NH_4Cl + NaOH \rightarrow NaCl + NH_3 + H_2O\). A challenge in this method is that the resulting ammonia gas has a strong smell and is harmful if inhaled.
05

Production of Carbon Dioxide (\(CO_2\))

Carbon dioxide can be made in the lab by reacting calcium carbonate (\(CaCO_3\)) with hydrochloric acid (\(HCl\)). The reaction is: \(CaCO_3 + 2HCl \rightarrow CaCl_2 + CO_2 + H_2O\). The difficulty could be handling hydrochloric acid which is a strong acid and can cause burns.

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Most popular questions from this chapter

Write a plausible chemical equation to represent the reaction of \((\mathrm{a}) \mathrm{Cl}_{2}(\mathrm{g}) \quad\) with cold \(\quad \mathrm{NaOH}(\mathrm{aq})\) (b) \(\mathrm{NaI}(\mathrm{s})\) with hot \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { concd aq }) ;\) (c) \(\mathrm{Cl}_{2}(\mathrm{g})\) with \(\mathrm{KI}_{3}(\mathrm{aq}) ; \quad\) (d) \(\quad \mathrm{NaBr}(\mathrm{s}) \quad\) with hot \(\mathrm{H}_{3} \mathrm{PO}_{4}\) \((\text { concd aq })\) (e) \(\mathrm{NaHSO}_{3}(\mathrm{aq})\) with \(\mathrm{MnO}_{4}^{-1}(\mathrm{aq})\) in dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\).

Describe a chemical test you could use to determine whether a white solid is \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) or \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} .\) Explain the basis of this test using a chemical equation or equations.

The boiling points of oxygen and argon are \(-183^{\circ} \mathrm{C}\) and \(-189^{\circ} \mathrm{C},\) respectively. Because the boiling points are so similar, argon obtained from the fractional distillation of liquid air is contaminated with oxygen. The following three-step procedure can be used to obtain pure argon from the oxygen-contaminated sample: (1) Excess hydrogen is added to the mixture and then the mixture is ignited. (2) The mixture from step (1) is then passed over hot copper(II) oxide. (3) The mixture from step (2) is passed over a dehydrated zeolite material (see Chapter 21 ). Explain the purpose of each step, writing chemical equations for any reactions that occur.

In water, \(\mathrm{O}^{2-}\) is a strong base. If \(50.0 \mathrm{mg}\) of \(\mathrm{Li}_{2} \mathrm{O}\) is dissolved in \(750.0 \mathrm{mL}\) of aqueous solution, what will be the pH of the solution?

Use the following electrode potential diagram for basic solutions to classify each of the statements below as true or false. Assume standard conditions. $$\begin{aligned}\mathrm{SO}_{4}^{2-} \stackrel{-0.936 \mathrm{V}}{\longrightarrow} \mathrm{SO}_{3}^{2-} & \stackrel{-0.576 \mathrm{V}}{\longrightarrow} \\\& \mathrm{S}_{2} \mathrm{O}_{3}^{2-} \stackrel{-0.74 \mathrm{V}}{\longrightarrow} \mathrm{S} \stackrel{-0.476 \mathrm{V}}{\longrightarrow} \mathrm{S}^{2-}\end{aligned}$$ (a) Sulfate \(\left(\mathrm{SO}_{4}^{2-}\right)\) is a stronger oxidant than thiosulfate \(\left(\mathrm{S}_{2} \mathrm{O}_{3}^{2}\right)\) in basic solution. (b) \(S^{2-}\) can be used as a reducing agent in basic solutions. (c) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) is stable with respect to disproportionation to \(\mathrm{SO}_{3}^{2-}\) and \(\mathrm{S}\) in basic solution.
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