What are three examples of an endothermic reaction?

Melting ice cubes, melting solid salts, and sublimation of dry ice into carbon dioxide gas are three instances of endothermic reactions.

What is endothermic reaction give one example?

Endothermic reaction is a chemical reaction in which heat is absorbed. Temperatures drop as a result of it. e.g. Nitric oxide gas is generated when nitrogen and oxygen are heated to a temperature of around 3000°C.

What are endothermic and exothermic reaction?

The temperature of the immediate surroundings rises as an exothermic process releases heat. An endothermic process absorbs heat from the environment and cools it.

What type of reaction occurs in handwarmer?

In hand warmers, the chemical reaction is exothermic, which means it releases surplus energy as heat. As a result, you can warm your hands by combining a few chemicals.

Why self heating cans can only be used once?

Because the metal at the bottom of the can is coated with a heat-sensitive substance that reacts when it comes into touch with food or drink, the self-heating can only be utilised once. The reaction initiates oxidation, a chemical reaction that causes the metal to dissolve and rust.

What happens when you put hand warmers in water?

A hand warmer is made up of sodium acetate that has been dissolved in water. The solution has been heated to dissolve more sodium acetate, making it'super-saturated.' The solution rapidly crystallises.

Endothermic Reaction Examples with Equations

Table of Contents

Endothermic Reaction

When a chemical link is broken, energy is normally released in the process. The creation of chemical bonds, too, necessitates an energy input. The energy that is supplied/released can take many different forms (such as heat, light, and electricity). Endothermic reactions are characterised by the creation of chemical bonds as a result of heat absorption from the environment. Exothermic reactions, on the other hand, involve the release of heat energy generated by bond-breakage.

What is Endothermic Process?

Endothermic reactions are chemical processes in which the reactants absorb heat from the environment to produce products. These reactions cause a cooling effect by lowering the temperature of the surrounding environment. Ice cubes absorb heat energy from their surroundings and melt to generate liquid water, which is an endothermic process.

Endothermic Process for Class 10 Students

A chemical process that is generally accompanied by the retention of warmth (or heat), or a living being that creates warmth (or heat) to maintain its temperature, is known as an endothermic reaction. A chemical process that operates only if heat is retained is an example of an endothermic process reaction. A warm-blooded animal, such as humans, is an example of an endothermic mammal.

Endothermic processes require energy from the surrounding environment, preferably in the form of heat, in order to occur. Because endothermic processes absorb heat from their surroundings, they will produce a slight drop in temperature in their surroundings. They’re also non-spontaneous since endothermic reactions produce products that have more energy than the reactants. As a result, the enthalpy adjustment for an endothermic process is always positive. Heat is necessary for a chemical reaction involving the dissolution of ice, hence the process is endothermic. The concept is also commonly employed in physical disciplines, such as in chemical reactions, where warm energy (heat) is converted to chemical bond energy.

Endothermic Reaction Equations for Class 10

Reactants + Energy —> Products

is the general equation for an endothermic reaction. Note that H stands for energy change. The temperature of the products in endothermic reactions is usually lower than the temperature of the reactants.

Melting ice cubes, solid salts, liquid water evaporation, and frost to water vapour conversion (melting, boiling, and evaporation are all endothermic processes).

10 Examples of Endothermic Reactions with Equations

Endothermic reactions are chemical reactions that absorb heat energy from their surroundings, resulting in a decrease in temperature. Here are 10 examples of endothermic reactions along with their balanced chemical equations:

Melting of ice: H2O(s) → H2O(l) Heat is absorbed to convert ice into liquid water.
Dissolving ammonium nitrate in water: NH4NO3(s) + H2O(l) → NH4NO3(aq) The dissolution process absorbs heat.
Photosynthesis: 6 CO2(g) + 6 H2O(l) + light energy → C6H12O6(aq) + 6 O2(g) Photosynthesis in plants is an endothermic process because it requires energy from sunlight.
Thermal decomposition of calcium carbonate: CaCO3(s) → CaO(s) + CO2(g) Heat is needed to break down calcium carbonate into calcium oxide and carbon dioxide.
Ammonium chloride and water: NH4Cl(s) + H2O(l) → NH4Cl(aq) Dissolving ammonium chloride in water absorbs heat.
Electrolysis of water: 2 H2O(l) → 2 H2(g) + O2(g) Electrolysis of water requires an input of electrical energy, making it endothermic.
Reaction between barium hydroxide and ammonium thiocyanate: Ba(OH)2(aq) + 2 NH4SCN(aq) → Ba(SCN)2(aq) + 2 NH4OH(aq) Mixing barium hydroxide and ammonium thiocyanate results in an endothermic reaction.
Sublimation of dry ice (solid carbon dioxide): CO2(s) → CO2(g) Dry ice sublimates at a temperature below room temperature, absorbing heat.
Thermal decomposition of hydrogen peroxide: 2 H2O2(l) → 2 H2O(l) + O2(g) Breaking down hydrogen peroxide into water and oxygen requires heat.
Reaction between ammonium nitrate and water: NH4NO3(s) + H2O(l) → NH4+ (aq) + NO3− (aq) Dissolving ammonium nitrate in water is an endothermic process.

These reactions all involve the absorption of energy in the form of heat or other forms (such as light or electricity) from their surroundings, resulting in a decrease in temperature.

Endothermic Reaction Process Formula for Class 10

In photosynthesis, plants are make the simple sugar glucose (C₆H₁₂O₆) from carbon dioxide (CO₂) and water (H₂O). They also release oxygen (O₂) in the process. The reactions of photosynthesis are summed up by.

6 CO₂ + 6 H₂O → C₆H₁₂O₆ + 6 O₂

Example of Endothermic Reaction Class 10

Endothermic reactions are chemical reactions that absorb heat from their surroundings, resulting in a decrease in temperature. In these reactions, energy is required to break the existing bonds in the reactants, which is greater than the energy released when new bonds are formed in the products. As a result, they feel cold to the touch and usually occur with the input of heat. Here are some examples of endothermic reactions:

Dissolution of Ammonium Nitrate: When ammonium nitrate (NH4NO3) dissolves in water, it absorbs heat from the surroundings, causing the temperature of the solution to decrease. This reaction is often used in instant cold packs.
Photosynthesis: Photosynthesis is an important biological endothermic process that occurs in plants. Carbon dioxide and water are converted into glucose and oxygen in the presence of sunlight. This process absorbs energy from the sun, making it endothermic.
Electrolysis of Water: When electricity is passed through water (H2O), it undergoes electrolysis to produce hydrogen gas (H2) and oxygen gas (O2). This process is endothermic because it requires energy input to break the bonds in water molecules.
Melting Ice: The process of ice melting into liquid water is also an endothermic reaction. Energy is absorbed from the surroundings to break the hydrogen bonds holding the ice lattice together.
Evaporation: When a liquid, such as water, evaporates into a gas, it absorbs heat from the surroundings. This is why you feel cold when sweat evaporates from your skin.
Baking Soda and Vinegar Reaction: Mixing baking soda (sodium bicarbonate, NaHCO3) and vinegar (acetic acid, CH3COOH) results in a chemical reaction that produces carbon dioxide gas (CO2), water (H2O), and sodium acetate (CH3COONa). This reaction is endothermic and feels cold to the touch.
Ammunition Decomposition: Some types of ammunition or explosives undergo endothermic reactions when they decompose. For example, ammonium perchlorate (NH4ClO4) decomposes endothermically when ignited.
Reaction of Barium Hydroxide Octahydrate with Ammonium Chloride: Mixing solid barium hydroxide octahydrate (Ba(OH)2·8H2O) with solid ammonium chloride (NH4Cl) results in an endothermic reaction. It absorbs heat from the surroundings and causes a decrease in temperature.
Thermal Decomposition of Calcium Carbonate: When calcium carbonate (CaCO3) is heated, it decomposes into calcium oxide (CaO) and carbon dioxide (CO2). This decomposition reaction is endothermic and requires heat input to proceed.

These are just a few examples of endothermic reactions, and there are many more in chemistry and biology. Endothermic reactions are characterized by a decrease in temperature and the absorption of energy from their surroundings.

Endothermic Reaction Examples in Real Life

Sublimation of solid CO₂
Evaporation of liquid water, formation of water vapour.
The baking of bread.
The melting of ice to form water.

To keep cool, the human body uses the endothermic characteristic of evaporation. Sweating serves as a means of accomplishing this. Sweat (formed on the skin’s surface) absorbs heat from the skin and evaporates, resulting in a cooling effect.

Sweating, on the other hand, is not an exothermic response. Existing chemical bonds can be broken, new chemical bonds can be formed, or both can happen in a chemical reaction. Sweat evaporation does not result in any chemical changes, but it does result in a physical phase shift (from liquid to vapour). As a result, evaporation is classified as a physical rather than an endothermic reaction.

Examples of Endothermic Reactions vs. Exothermic Reactions

The phrases ‘Endo’ and ‘Exo,’ which imply ‘inside’ and ‘out,’ respectivelyGreek roots. The major difference between endothermic and exothermic reactions, as their names suggest, is that the former absorbs heat from the environment while the latter releases it.

An endothermic process is one that absorbs heat from its environment. As a result, all endothermic reactions and processes are endothermic. The opposite, however, is not true. Physical rather than chemical changes are involved in many endothermic reactions.

S. No.	ENDOTHERMIC REACTION	EXOTHERMIC REACTION
1.	The system absorbs heat from the surroundings	The system releases heat into the surroundings
2.	The entropy of the surrounding decreases, i.e. => ΔS <0	Entropy of the surrounding increases, i.e. => ΔS>0
3.	Enthalpy change (ΔH) is positive	Enthalpy change (ΔH) is negative