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Chapter 22: Problem 81

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.

Short Answer

Expert verified
In this three-step purification process, the first step is the combustion of oxygen with hydrogen to form water, removing oxygen from the mixture. In the second step, any residual hydrogen is reacted with copper(II) oxide to form water and copper, removing hydrogen from the mixture. Then the third step is passing the remaining mixture over a dehydrated zeolite material to adsorb water, leaving pure argon.

Step by step solution

01

Understanding Step 1

In the first step, excess hydrogen is added to the mixture and ignited. The purpose of this step is to react oxygen in the mixture with hydrogen to form water. This is a basic combustion reaction in which oxygen reacts with hydrogen to produce water. The reaction equation: \[2H_2(g) + O_2(g) \rightarrow 2H_2O(g)\]
02

Understanding Step 2

In the second step, the mixture from the previous step is passed over hot copper(II) oxide. The purpose here is to ensure all hydrogen is removed. Any surplus hydrogen from the previous step reacts with copper(II) oxide to produce water and copper. Here is the chemical equation for this reaction: \[H_2(g) + CuO(s) \rightarrow H_2O(g) + Cu(s)\]. In this step, water will be also produced and turned into steam due to the heat.
03

Understanding Step 3

In the third step, the mixture from step 2 is passed over a dehydrated zeolite material. Zeolite being a porous material, is used because it has the ability to adsorb water. The remaining substance will be pure argon, since oxygen and hydrogen have been removed in the form of water.

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Most popular questions from this chapter

Despite the fact that it has the higher molecular mass, XeO \(_{4}\) exists as a gas at \(298 \mathrm{K},\) whereas \(\mathrm{XeO}_{3}\) is a solid. Give a plausible explanation for this observation.

Suppose that the sulfur present in seawater as \(\mathrm{SO}_{4}^{2-}\) \(\left(2650 \mathrm{mg} \mathrm{L}^{-1}\right)\) could be recovered as elemental sulfur. If this sulfur were then converted to \(\mathrm{H}_{2} \mathrm{SO}_{4},\) how many cubic kilometers of seawater would have to be processed to yield the average U.S. annual consumption of about 45 million tons of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

Show how you would use elemental sulfur, chlorine gas, metallic sodium, water, and air to produce aqueous solutions containing (a) \(\mathrm{Na}_{2} \mathrm{SO}_{3} ;\) (b) \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} .\) [Hint: You will have to use information from other chapters as well as this one.].

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) \(\mathrm{NO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\)

Use VSEPR theory to predict the probable geometric structures of (a) \(\mathrm{XeO}_{3} ;\) (b) \(\mathrm{XeO}_{4} ;\) (c) \(\mathrm{XeF}_{5}^{+}\).
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