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Chapter 11: Problem 2

Describe how you could purify iodine by sublimation.

Short Answer

Expert verified
Purify iodine by sublimating it and then condensing the vapors as crystals on a cooler surface.

Step by step solution

01

Understand Sublimation

Sublimation is a process where a solid turns directly into a gas without passing through the liquid phase. Iodine has the property of sublimating when heated slightly, turning from a solid directly into iodine vapor.
02

Setup the Apparatus

Prepare a sublimation apparatus. Place the solid iodine in an evaporating dish and cover it with an inverted funnel. The narrow end of the funnel should point upwards. Place a filter paper inside the funnel to catch the purified iodine vapors.
03

Heat the Iodine

Gently heat the evaporating dish containing the iodine. The heat should be even and not too intense to avoid melting the iodine.
04

Collect Sublimated Iodine

As the iodine begins to sublime, it will transform into a gas and rise into the funnel, where it will cool and deposit as purified iodine crystals on the cooler surfaces, such as the filter paper inside the funnel.
05

Retrieve Purified Iodine

After the heating process, allow the apparatus to cool down before carefully removing the filter paper. The iodine crystals that have sublimed and re-deposited on the cooler surface of the filter paper are now purified.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Purification of Iodine
Purification of iodine through sublimation is a simple and effective technique commonly used in chemistry labs to obtain pure iodine. Unlike other compounds, iodine has a unique ability to transition directly from its solid form to a gaseous state, which is particularly useful for separating pure iodine from impurities that do not sublime. When iodine is heated gently, it sublimes, allowing us to collect the iodine vapors away from non-volatile contaminants. This process results in the deposition of pure iodine crystals while the impurities remain in the original container.
Solid to Gas Transition
The solid to gas transition, also known as sublimation, involves a substance changing directly from a solid to a gas without going through a liquid phase. This is a characteristic of iodine and some other substances, such as dry ice (solid carbon dioxide). The key to sublimation is that the pressure and temperature conditions must be just right. Iodine sublimates easily when slightly heated because it overcomes the atmospheric pressure and enters the gaseous phase directly. This transition is particularly used for purification purposes because it allows the separation of substances based on their ability to sublime.
Sublimation Apparatus
A sublimation apparatus is a simple setup used to facilitate the sublimation process. The basic components are:
  • An evaporating dish to hold the solid iodine.
  • An inverted funnel placed on top of the dish, acting as the chamber for the iodine vapor to rise.
  • A piece of filter paper embedded inside the funnel to capture the purified crystals.
The evaporating dish is gently heated to initiate sublimation, while the funnel directs the iodine vapor upwards. The narrow end of the funnel channels the gas, where the temperature is cooler, leading to the deposition of pure iodine crystals on the filter paper as it condenses back into solid form.
Chemical Separation Techniques
Chemical separation techniques are essential methods in chemistry for isolating, purifying, and identifying different substances within a mixture. Sublimation is a phase transition technique that is helpful for substances that can easily switch from a solid to a gas. It differs from other separation methods, such as distillation, crystallization, or filtration, by exploiting the unique thermal properties of certain compounds. This method is valued for its ability to purify without the need for solvents, making it an eco-friendly approach. Each separation technique has its advantages and is chosen based on the specific properties of the components involved.

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Most popular questions from this chapter

Metallic barium has a body-centered cubic structure (all atoms at the lattice points) and a density of \(3.51 \mathrm{~g} / \mathrm{cm}^{3}\). Assume barium atoms to be spheres. The spheres in a bodycentered array occupy \(68.0 \%\) of the total space. Find the atomic radius of barium. (See Problem 11.87.)

A quantity of ice at \(0.0^{\circ} \mathrm{C}\) was added to \(33.6 \mathrm{~g}\) of water at \(21.0^{\circ} \mathrm{C}\) to give water at \(0.0^{\circ} \mathrm{C}\). How much ice was added? The heat of fusion of water is \(6.01 \mathrm{~kJ} / \mathrm{mol}\) and the specific heat is \(4.18 \mathrm{~J} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\)

Use chemical principles to discuss the following observations: a. \(\mathrm{CO}_{2}\) sublimes at \(-78^{\circ} \mathrm{C}\), whereas \(\mathrm{SiO}_{2}\) boils at \(2200^{\circ} \mathrm{C}\). b. HF boils at \(19^{\circ} \mathrm{C}\), whereas \(\mathrm{HCl}\) boils at \(-85^{\circ} \mathrm{C}\). c. \(\mathrm{CF}_{4}\) boils at \(-128^{\circ} \mathrm{C}\), whereas \(\mathrm{SiF}_{4}\) boils at \(-86^{\circ} \mathrm{C}\).

Metallic magnesium has a hexagonal close-packed structure and a density of \(1.74 \mathrm{~g} / \mathrm{cm}^{3}\). Assume magnesium atoms to be spheres of radius \(r\). Because magnesium has a close-packed structure, \(74.1 \%\) of the space is occupied by atoms. Calculate the volume of each atom; then find the atomic radius, \(r\). The volume of a sphere is equal to \(4 \pi r^{3} / 3\).

Identify the phase transition occurring in each of the following. a. The water level in an aquarium tank falls continuously (the tank has no leak). b. A mixture of scrambled eggs placed in a cold vacuum chamber slowly turns to a powdery solid. c. Chlorine gas is passed into a very cold test tube where it turns to a yellow liquid. d. When carbon dioxide gas under pressure exits from a small orifice, it turns to a white "snow." e. Molten lava from a volcano cools and turns to solid rock.
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