Chlorine Reacts With Dry Slaked Lime: What Happens?

When chlorine gas reacts with dry slaked lime (Ca(OH)2), it forms bleaching powder or calcium hypochlorite. This reaction is a crucial process in the chemical industry, leading to the production of a valuable compound with numerous applications.

Let’s delve a bit deeper into this fascinating reaction. Dry slaked lime, also known as calcium hydroxide, is a white powder that readily absorbs moisture from the air. When chlorine gas is passed over this powder, a series of chemical reactions occur, resulting in the formation of bleaching powder. This process involves the oxidation of calcium hydroxide by chlorine, leading to the formation of calcium hypochlorite. Calcium hypochlorite is the primary component of bleaching powder, responsible for its powerful bleaching and disinfecting properties.

The chemical equation for this reaction can be represented as follows:

2Ca(OH)2 + Cl2 → CaOCl2 + CaCl2 + 2H2O

Here, calcium hydroxide (Ca(OH)2) reacts with chlorine gas (Cl2) to produce calcium hypochlorite (CaOCl2), calcium chloride (CaCl2), and water (H2O). This reaction occurs at room temperature, and the resulting bleaching powder is a white powder with a characteristic chlorine-like odor.

Bleaching powder is widely used in various industries, including:

Textile Industry: Bleaching fabrics and removing stains.
Paper Industry: Whitening paper pulp.
Water Treatment: Disinfecting drinking water and swimming pools.
Sanitation: Disinfecting surfaces and killing bacteria.

This versatile compound plays a vital role in our daily lives, ensuring the cleanliness and hygiene of our surroundings.

You’re asking about bleaching powder, right? It’s a pretty interesting substance!

You get bleaching powder when you react chlorine with dry slaked lime. The chemical formula for bleaching powder is calcium oxychloride ($CaOCl_2$). It’s a really versatile substance. We use bleaching powder to clean clothes, whiten linen, and even bleach cotton in the textile industry.

So, how does bleaching powder work? Well, the chlorine in the bleaching powder is actually what does the bleaching. It acts as an oxidizing agent, which means it removes color from things. This is why bleaching powder is so good at cleaning clothes and whitening linen.

There’s a little more to the story. Bleaching powder is actually a mixture of calcium hypochlorite ($Ca(OCl)_2$), calcium chloride ($CaCl_2$), and calcium hydroxide ($Ca(OH)_2$). The calcium hypochlorite is the main ingredient that does the bleaching. But the other ingredients are important too. They help to stabilize the bleaching powder and make it easier to store and use.

Bleaching powder can be a bit tricky to handle, though. It’s a strong oxidizer, so it’s important to use it carefully. You should always wear gloves and eye protection when handling bleaching powder. You also need to store it in a cool, dry place, away from direct sunlight.

If you’re ever wondering what the white powder in your laundry detergent is, it’s probably bleaching powder! It’s a pretty common ingredient in many household cleaning products.

You’re asking about the reaction between slaked lime (calcium hydroxide) and chlorine gas. This reaction is a classic example of how chlorine can act as an oxidizing agent.

The balanced chemical equation for this reaction is:

Ca(OH)₂ + Cl₂ → Ca(OCl)₂ + H₂O

In this reaction, chlorine gas reacts with calcium hydroxide to produce calcium hypochlorite (also known as bleaching powder) and water.

Let’s break down what’s happening:

Chlorine (Cl₂) acts as an oxidizing agent, meaning it gains electrons and gets reduced.
Calcium hydroxide (Ca(OH)₂) is the reducing agent, meaning it loses electrons and gets oxidized.
* The chlorine molecule (Cl₂) splits into two chlorine atoms (Cl).
* Each chlorine atom gains an electron from the hydroxide ion (OH⁻) in calcium hydroxide, forming a hypochlorite ion (OCl⁻).
* This process also releases a hydrogen ion (H⁺), which combines with another hydroxide ion to form water (H₂O).
* The calcium ions (Ca²⁺) combine with the hypochlorite ions (OCl⁻) to form calcium hypochlorite (Ca(OCl)₂).

So, in essence, the reaction involves the oxidation of calcium hydroxide and the reduction of chlorine, leading to the formation of calcium hypochlorite (bleaching powder) and water.

Here’s a bit more about the products:

Calcium hypochlorite (Ca(OCl)₂) is a white powder commonly used as a bleaching agent and a disinfectant due to its strong oxidizing properties.
Water (H₂O) is formed as a byproduct of the reaction.

This reaction highlights the versatility of chlorine, which can react with both metals and non-metals.

Let’s talk about the reaction of slaked lime. You’re probably wondering, what happens when quicklime (CaO) meets water? It’s a pretty interesting reaction, and it’s all about chemistry!

Quicklime (CaO) reacts with water to form slaked lime Ca(OH)2 and releases heat in the process. This reaction is represented by the following equation:

CaO (s) + H2O (l) ⟶ Ca(OH)2 (s) + Heat

This reaction is exothermic, which means it releases heat. You’ll actually feel the heat if you mix quicklime and water! The reaction is also quite vigorous, and it can even cause the mixture to boil.

Here’s a deeper dive into what’s going on:

Quicklime (CaO) is a white, powdery compound that’s very reactive. It’s also known as calcium oxide.
Water (H2O), of course, is the liquid we drink.
Slaked lime (Ca(OH)2) is also a white powder, but it’s less reactive than quicklime. It’s known as calcium hydroxide.

So, when quicklime and water mix, the water molecules react with the calcium oxide molecules. This breaks apart the calcium oxide molecules and creates calcium hydroxide molecules. The reaction also releases heat, which is why the mixture gets hot.

This reaction is a key part of many processes, including:

Mortar and concrete production: Slaked lime is used as a binder in mortar and concrete. The reaction with water helps to create a strong, durable material.
Treating acidic soil: Slaked lime can be added to acidic soil to neutralize the acidity and improve plant growth.
Water treatment: Slaked lime is used to soften water by removing calcium and magnesium ions.

You can see that this reaction is pretty important! It’s a great example of how chemistry can be used to create useful products and solve problems.

Dry slaked lime is a dry white powder made primarily from calcium hydroxide. It’s created by reacting lime with water. You might also hear it called slaked lime.

Imagine this: you take lime, which is basically calcium oxide (CaO). When you mix it with water, a chemical reaction happens. This reaction produces calcium hydroxide (Ca(OH)2) and releases heat. This process is called slaking.

The result of this reaction is dry slaked lime. This powder is a versatile material with a wide range of applications. You’ll find it in construction, agriculture, and even in the food industry!

Let’s break it down a bit further:

Lime: This is the starting material, usually obtained from limestone. It’s a hard, rocky substance.
Water: This is what triggers the chemical reaction with lime.
Slaking: This is the process of reacting lime with water to form calcium hydroxide. It’s like a controlled chemical reaction.
Dry Slaked Lime: This is the final product, a fine white powder that’s ready to be used.

Think of it like baking a cake. You start with ingredients like flour, sugar, and eggs. You then combine them, mix them, and bake them to create the final cake. Dry slaked lime is similar, only instead of using flour, sugar, and eggs, you use lime and water!

When calcium reacts with chlorine, it’s a fascinating chemical dance! Calcium, a generous giver, readily hands over two of its electrons. These electrons find a new home, one with each chlorine atom. This exchange creates a new kind of family, a calcium ion with a positive 2 charge (Ca+2) and two chloride ions, each with a negative 1 charge (Cl-).

These ions, now oppositely charged, are attracted to each other like magnets, forming a strong bond called an ionic bond. This bond is the glue that holds them together in a structured compound called calcium chloride (CaCl2). It’s like a tiny, organized dance where the positive calcium ion and the two negative chloride ions are always in perfect alignment, creating a stable and beautiful structure.

The reaction itself is quite vigorous, releasing a significant amount of heat energy and producing a bright white light. You might even hear a slight popping sound. This is because the formation of the ionic bond releases a lot of energy, often enough to excite the electrons in the newly formed calcium chloride, causing them to emit light.

Let’s break down the process in more detail.

Calcium (Ca), being in group 2 of the periodic table, has two valence electrons in its outermost shell. These electrons are relatively loosely bound to the atom and are easily lost.
Chlorine (Cl), being in group 17, has seven valence electrons in its outermost shell. It needs only one more electron to achieve a stable octet configuration.
* When calcium and chlorine react, the two valence electrons of calcium are transferred to two chlorine atoms, one electron to each chlorine atom.
* This transfer of electrons results in the formation of positive calcium ions (Ca+2) and negative chloride ions (Cl-).
* The electrostatic attraction between the oppositely charged ions results in the formation of an ionic bond, creating the compound calcium chloride (CaCl2).

This process, called ionic bonding, is fundamental to understanding the formation of many inorganic compounds. It showcases the power of electron transfer and the forces that govern the formation of matter around us.

When hydrogen gas is passed through dry slaked lime, nothing happens. Slaked lime is calcium hydroxide, and it’s a solid. Hydrogen gas is a very small molecule, and it won’t react with calcium hydroxide in this way.

You’re probably thinking about the reaction of chlorine gas with slaked lime, which produces bleaching powder. This is a very important reaction, and it’s used to make a variety of household and industrial products.

Here’s what happens:

Chlorine gas (Cl2) is reacted with slaked lime (Ca(OH)2).
* The chlorine gas reacts with the calcium hydroxide, forming calcium hypochlorite (Ca(OCl)2) and water (H2O):

Ca(OH)2 + Cl2 → Ca(OCl)2 + H2O

* Calcium hypochlorite is the active ingredient in bleaching powder. It’s a powerful oxidizing agent and is used as a disinfectant, bleaching agent, and deodorant.

Let me explain why hydrogen gas doesn’t react with slaked lime the same way chlorine does. Hydrogen gas isn’t as reactive as chlorine gas. It doesn’t readily form bonds with other elements like chlorine does. Plus, calcium hydroxide is quite stable and doesn’t easily break down or react with hydrogen.

So, while chlorine and slaked lime react to create bleaching powder, hydrogen gas just passes through slaked lime without any reaction.

Let’s break down the chemical reaction that happens when chlorine gas reacts with dry slaked lime.

Bleaching powder is formed when chlorine gas reacts with dry slaked lime, also known as calcium hydroxide. This reaction produces a white powder that’s widely used as a bleaching agent and a disinfectant.

Here’s a more detailed explanation of the process:

1. The Reaction: The reaction between chlorine gas (Cl2) and calcium hydroxide (Ca(OH)2) is a chlorination reaction. Chlorine gas is bubbled through a suspension of dry slaked lime, and the chlorine atoms react with the hydroxide ions in the calcium hydroxide.

2. Formation of Hypochlorite: This reaction leads to the formation of calcium hypochlorite (Ca(ClO)2) which is the key component of bleaching powder. Calcium hypochlorite is a powerful oxidizing agent, which means it can readily accept electrons from other substances. This is the reason why it is so effective in breaking down colored compounds and killing bacteria.

3. Additional Products: The reaction also produces other byproducts such as calcium chloride (CaCl2). However, calcium hypochlorite is the main product and the one that gives bleaching powder its distinctive properties.

4. The Chemical Equation: The reaction can be represented by the following chemical equation:

2 Ca(OH)2 + 2 Cl2 → Ca(ClO)2 + CaCl2 + 2 H2O

Bleaching powder is a versatile and important chemical compound. Its applications extend far beyond its use in the laundry. Here are some examples:

Water Treatment: Bleaching powder is frequently used to disinfect water supplies, killing harmful bacteria and making it safe for drinking.
Sanitization: It’s employed in sanitation and hygiene products for disinfecting surfaces and killing germs.
Paper Production: Bleaching powder plays a crucial role in the paper industry, helping to bleach pulp and make white paper.
Textile Industry: It’s used to bleach fabrics, giving them a brighter and more appealing appearance.

Let me know if you have any other questions about the chemistry of bleaching powder!

Let’s explore what happens when dry slaked lime reacts with chlorine.

Dry slaked lime, also known as calcium hydroxide (Ca(OH)2), reacts with chlorine gas (Cl2) to produce bleaching powder, a compound with the chemical formula CaOCl2. This process is a crucial step in the production of a widely used disinfectant and bleaching agent.

The reaction involves the absorption of chlorine by calcium hydroxide. This reaction occurs when chlorine gas is passed over dry slaked lime, and it results in a compound that contains both calcium hypochlorite (Ca(OCl)2) and calcium chloride (CaCl2). This mixture is what we know as bleaching powder.

The reaction can be represented by the following equation:

Ca(OH)2 + Cl2 → CaOCl2 + H2O

Bleaching powder is a pale yellowish powder with a strong chlorine-like odor. It’s commonly used for:

Disinfecting water: Bleaching powder effectively kills bacteria and viruses in water, making it safe for drinking.
Bleaching textiles: The compound is a powerful bleaching agent that whitens fabrics and removes stains.
Sanitizing surfaces: Bleaching powder is used to disinfect surfaces in homes, hospitals, and other areas.

Now, let’s answer the question about what happens when Cl reacts with dry slaked lime.

You are correct that calcium oxide (CaO), also known as quick lime, reacts with water to form calcium hydroxide (Ca(OH)2). This is a separate reaction that takes place before the formation of bleaching powder.

Quick lime (CaO) is a white, powdery substance. When quick lime comes into contact with water, it undergoes a highly exothermic reaction. The reaction releases heat, and the quick lime dissolves in the water, forming calcium hydroxide (Ca(OH)2). This process is known as slaking.

CaO + H2O → Ca(OH)2 + Heat

The calcium hydroxide (Ca(OH)2) formed in this reaction is then used to react with chlorine gas (Cl2) to produce bleaching powder, as we described earlier. So, the two reactions are interconnected and essential for the production of this valuable chemical.

Let’s dive into what happens when chlorine is passed over slaked lime!

You’re right, this reaction is pretty cool. When you pass chlorine gas over slaked lime (calcium hydroxide, Ca(OH)2), which is at a temperature of around 313 K (40°C), the chlorine gets absorbed quickly. This reaction forms bleaching powder, also known as calcium oxychloride.

Here’s the breakdown:

Slaked lime is a white powder that’s made by adding water to quicklime (calcium oxide).
* When chlorine gas reacts with slaked lime, a complex reaction occurs where chlorine gets incorporated into the slaked lime structure.
* This reaction produces bleaching powder (CaOCl2), which is a yellowish-white powder.

Bleaching powder is a powerful oxidizer, which means it can remove color from things. It’s widely used in various industries like paper and textiles for bleaching purposes. But that’s not all! Bleaching powder is also a disinfectant and is used in water treatment to kill harmful bacteria.

The reaction between chlorine and slaked lime can be represented by the following chemical equation:

2Ca(OH)2 + Cl2 → CaOCl2 + CaCl2 + 2H2O

This equation shows how chlorine (Cl2) reacts with slaked lime (Ca(OH)2) to form bleaching powder (CaOCl2), along with calcium chloride (CaCl2) and water (H2O).

Now, let’s talk about the magic behind bleaching action. Bleaching powder contains a unique combination of hypochlorite ions (OCl-) and chloride ions (Cl-). When bleaching powder is dissolved in water, it releases hypochlorite ions. These ions are super reactive and can break down colored compounds, making them colorless. The bleaching process essentially involves the oxidation of the colored compounds by hypochlorite ions.

Think of it like this: the hypochlorite ions grab electrons from the colored compounds, changing their structure and turning them colorless. Pretty neat, right?

So, the next time you see a bright white piece of paper or a crisp white shirt, remember that bleaching powder might have played a role in achieving that dazzling whiteness!

You’re curious about what happens when chlorine reacts with dry slaked lime, also known as calcium hydroxide. It’s a pretty cool reaction that results in a very useful product!

Chlorine reacts with dry slaked lime to create bleaching powder, which is also called calcium hypochlorite. It’s a white powder that’s commonly used as a disinfectant and bleaching agent.

Let’s break down the process a bit more:

When you mix chlorine gas (Cl₂) with dry slaked lime (Ca(OH)₂), a chemical reaction takes place. The chlorine reacts with the calcium hydroxide to form calcium hypochlorite (Ca(ClO)₂) and calcium chloride (CaCl₂). This reaction is best described by the following chemical equation:

2Ca(OH)₂ + 2Cl₂ → Ca(ClO)₂ + CaCl₂ + 2H₂O

The calcium hypochlorite is the active ingredient in bleaching powder. It’s the part that gives the powder its bleaching and disinfecting properties. Calcium chloride is a byproduct of the reaction and is not as active.

Here’s a bit more about bleaching powder:

Bleaching powder is widely used in various industries, including:
Textile industry: For bleaching fabrics
Paper industry: For bleaching pulp
Water treatment: For disinfecting water
Sanitation: For disinfecting surfaces and toilets
Bleaching powder releases chlorine when it dissolves in water. This chlorine is what actually does the bleaching and disinfecting.
* It’s important to use bleaching powder carefully because it can be irritating to the skin, eyes, and respiratory system. It should always be stored in a dry, cool place and handled with caution.

This reaction of chlorine with dry slaked lime is a fascinating example of how chemistry can be used to create products that benefit our lives.

Let’s dive into what happens when slaked lime isn’t completely dry.

When chlorine gas reacts with dry slaked lime, we get bleaching powder. This powder is a handy disinfectant and a key ingredient in many cleaning products.

But what happens if the slaked lime isn’t dry? Well, things change a bit. Instead of reacting directly with the slaked lime, chlorine gas reacts with the water present. This reaction forms hydrochloric acid and hypochlorous acid. These acids aren’t ideal for the reaction because they can affect the effectiveness of bleaching powder.

Now, let’s talk about slaked lime itself. It’s just calcium hydroxide, Ca(OH)2. It’s a white, powdery substance that is made by adding water to quicklime, CaO. This process is called “slaking.”

Remember, for the reaction with chlorine gas to produce bleaching powder, the slaked lime needs to be as dry as possible. If it’s not, it can hinder the reaction, resulting in lower yields of bleaching powder.

So, why is dryness so important? It all comes down to the chemistry of the reaction. Chlorine gas reacts with the hydroxyl ions (OH-) present in slaked lime, which are responsible for the formation of bleaching powder. When water is present, the chlorine gas preferentially reacts with the water molecules, forming hydrochloric acid and hypochlorous acid.

Think of it like this: Imagine you are trying to make a cake. You need all the ingredients to be in the right proportions for it to turn out well. In this case, the dry slaked lime is the key ingredient for a good batch of bleaching powder.

Let me know if you have any other questions about slaked lime or bleaching powder.

What happens when chlorine reacts in slaked lime? Chemistry

Reaction of chlorine with slaked lime: When chlorine Cl 2 is passed over slaked lime, it results in the formation of bleaching powder CaOCl 2. The reaction is as follows: Cl 2 g Chlorine + Ca OH 2 aq Slaked lime → CaOCl 2 aq Bleaching powder + H 2 O l Water. BYJU’S

What happens when chlorine is passed over slaked lime at

The reaction of chlorine with dry slaked lime produces bleaching powder, which is calcium oxychloride. Uses of bleaching powder: It is used in the paper and textile industries as a BYJU’S

What happen when Cl reacts with dry slaked lime? – Toppr

What happen when Cl reacts with dry slaked lime? Solution. Verified by Toppr. Dry slaked lime with reacts with chlorine to prepare bleaching powder. Cl2 + Ca(OH)2 Dry slaked Toppr

Slaked lime reacts with chlorine to give: – Vedantu

If the slaked lime is not dry, then chlorine reacts with water to form hydrochloric acid and hypochlorus acid. \[\begin{array}{l} {\rm{ C}}{{\rm{l}}_2} + Vedantu

What happens when Cl reacts with dry slaked lime? – Vedantu

What happens when Cl reacts with dry slaked lime?. Ans: Hint: It is a pale yellowish powder existing with a strong smell of chlorine. It is soluble in water but due to Vedantu

Slaked lime reacts with chlorine to give: – Vedantu

Let us a quick look towards the reaction of slaked lime with chlorine; Slaked lime i.e. calcium hydroxide when reacts with dry slaked lime gives a mixture of two Vedantu

Slaked Lime: Learn its Formula, Formation, Reactions, & Uses

Reaction of Slaked Lime. Given below are some of the reactions of slaked lime: Action of Heat: On heating, slaked lime loses water only at temperatures greater Testbook

what happen when dry chlorine gas passed through slaked lime

1. Dry chlorine gas is passed through slaked lime (calcium hydroxide). Step 2/6 2. Chlorine gas reacts with calcium hydroxide to form calcium hypochlorite and calcium Numerade

What happens when Cl reacts with dry slaked lime?

On the reaction of chlorine gas on dry slaked lime, bleaching powder is formed. The reaction is as follows- Bleaching powder, or calcium oxychloride, is the result of the infinitylearn.com

What happens when chlorine reacts with dry slaked lime – EMBIBE

When chlorine gas is passed through slakedlime calcium chloride and calcium hypochlorite is formed The following reaction will takeplace when calcium hydroxide is treated with embibe.com