Chapter 9: Problem 4

What is lime? What is the principle involved in the preparation of lime?

Short Answer

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Answer: The principle involved in the preparation of lime is calcination, a thermal treatment process in which limestone (calcium carbonate) is heated at high temperatures (900-1000°C) in the absence of air to decompose it into calcium oxide (lime) and carbon dioxide gas. The steps in the process are: 1) obtaining limestone, 2) crushing the limestone, 3) heating the limestone, 4) undergoing the calcination process, and 5) collecting and storing the resulting lime.

Step by step solution

Definition of Lime

Lime, also known as calcium oxide (CaO), is a white crystalline solid material widely used in the construction, steel, chemical, and agricultural industries. It is an inorganic compound derived from limestone, chalk, or other calcium-rich sources.

Preparation of Lime

The preparation of lime involves the process of calcination. Calcination is a thermal treatment process in which a solid substance, in this case, limestone or calcium carbonate (CaCO_3), is heated at high temperatures (approximately 900-1000°C) in the absence of air to cause its decomposition, forming calcium oxide (CaO) and releasing carbon dioxide (CO_2) as a byproduct.

Obtain Limestone

First, obtain a sample of limestone (calcium carbonate) from a naturally occurring source like limestone rock, chalk, or marble. Make sure it is free from impurities such as soil and other minerals.

Crush the Limestone

In order to facilitate the calcination process, crush the limestone into smaller pieces. The smaller particle size will allow for more efficient heating and a faster chemical reaction.

Heat the Limestone

Place the crushed limestone in a furnace or kiln and heat it at temperatures between 900 and 1000°C. Make sure the heating process occurs in the absence of air, as the presence of air can lead to the formation of undesirable products.

Calcination Process

During the heating process or calcination, calcium carbonate (CaCO_3) breaks down into calcium oxide (CaO) and carbon dioxide (CO_2). The chemical equation for this process can be represented as: CaCO_3 (s) ⟶ CaO (s) + CO_2 (g) The solid calcium oxide (or quicklime) is collected, while the carbon dioxide gas is released as a byproduct of the reaction.

Collect and Store Lime

Once the calcination process is complete, allow the calcium oxide (lime) to cool down, and then collect it. Store the resulting lime in a dry and airtight container to prevent it from reacting with moisture in the air, which can form calcium hydroxide (slaked lime). In summary, lime or calcium oxide (CaO) is prepared through the calcination of limestone or calcium carbonate (CaCO_3) at high temperatures in the absence of air. This process involves the decomposition of limestone into calcium oxide and the release of carbon dioxide as a byproduct.

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What is lime? What is the principle involved in the preparation of lime?

Short Answer

Step by step solution

Definition of Lime

Preparation of Lime

Obtain Limestone

Crush the Limestone

Heat the Limestone

Calcination Process

Collect and Store Lime

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