Login Get started

CHEMICAL REACTIONS AND EQUATIONS in 1 Shot: FULL CHAPTER COVERAGE (Concepts+PYQs) | Class 10 Boards

Physics Wallah Foundation・169 minutes read

Sunil Bhaiya explains chemical reactions, balancing equations, types of reactions, and practical applications, emphasizing the importance of various concepts and examples in understanding chemistry. The lesson also covers topics like physical and chemical changes, combustion, endothermic reactions, catalysts, decomposition reactions, and the importance of following NCERT guidelines for exams.

Insights

The lesson focuses on chemical reactions and equations, covering topics like characteristic balancing, types of reactions, and redox reactions.
Physical and chemical changes are distinguished, emphasizing changes in chemical composition.
Chemical reactions involve visible indicators like color changes and the formation of insoluble solids.
The importance of balancing chemical equations to respect the Law of Conservation of Mass is stressed.
Catalysts play a crucial role in accelerating or slowing down reactions, with examples of positive and negative catalysts provided.

Get key ideas from YouTube videos. It’s free

Recent questions

What is the difference between physical and chemical changes?
Physical changes involve altering the appearance without changing the composition, like melting ice. Chemical changes result in new substances forming, such as burning a candle.
How can chemical reactions be identified?
Chemical reactions can be identified by indicators like color changes, formation of precipitates, evolution of gas, or changes in temperature.
Why is balancing a chemical equation important?
Balancing a chemical equation ensures the Law of Conservation of Mass is respected, maintaining the same number of atoms on both sides of the equation.
What are some examples of decomposition reactions?
Decomposition reactions involve a single compound breaking into two or more products with the input of energy, like heat, electricity, or sunlight.
What is the role of catalysts in chemical reactions?
Catalysts can either speed up reactions (positive catalysts) or slow them down (negative catalysts) without being consumed, influencing the reaction rate significantly.

Related videos

Summary

00:00

"Live Physics Platform: Chemical Reactions Lesson"

The platform is introduced as the largest live tuning platform for physics.
The host, Sunil Bhaiya, greets the audience and initiates a chant of "Bharat Mata Ki Jai."
Sunil Bhaiya announces the topic for the day's lesson: chemical reactions and equations.
The lesson will cover topics like characteristic balancing, types of reactions, and redox reactions.
Students are advised to have a notebook, pen, NCERT book, food, and water for the lesson.
Sunil Bhaiya promises to teach theory and concepts, covering NCERT activities and questions.
The lesson will include examples and practical applications of the covered topics.
The distinction between physical and chemical changes is explained, emphasizing changes in chemical composition.
Chemical reactions are defined as the process of chemical change, with examples like melting ice and boiling water.
Various examples are provided to illustrate physical changes (melting ice) and chemical changes (burning candle).

17:48

Forces, combustion, and chemical reactions explained

Compressive force flattened the cup, changing its shape.
Paper cups were compared to illustrate the impact of forces on objects.
Combustion involves a chemical reaction with oxygen, producing heat and light.
Burning paper exemplified the combustion process, creating new products.
Carbon forms charcoal when burned in the presence of oxygen.
Chemical reactions can be identified by visible indicators like color changes.
Mixing barium chloride and sodium sulfate results in a white insoluble solid.
Precipitation occurs when two solutions form an insoluble solid after a chemical reaction.
Baking soda and vinegar react to release carbon dioxide gas.
Changes in physical state and temperature indicate chemical reactions.

36:35

Heat in Chemical Reactions: Absorption and Release

When a chemical reaction occurs, heat is absorbed from the surroundings, causing the temperature of the surroundings to decrease.
Heat energy is released into the surroundings when a substance burns, leading to an increase in the temperature of the immediate surroundings.
The process of releasing heat energy into the surroundings is known as endothermic reaction.
In reactions involving heat energy, it is crucial to consider not only heat but also other forms of energy.
Photosynthesis is a process where sunlight is used to synthesize carbon dioxide and water into glucose and oxygen, requiring energy input.
Decomposition of vegetable matter into compost involves a reaction that produces heat energy, increasing the temperature of the immediate surroundings.
Rusting of iron is a type of corrosion where iron reacts with water and oxygen, forming a layer of rust due to a slow chemical change.
Respiration is considered an exothermic reaction as it releases energy, particularly in the form of ATP, crucial for bodily functions.
Understanding the reactivity series helps determine the reactivity of metals like zinc, which reacts with acids such as dilute hydrochloric acid.
In exam scenarios, it is essential to understand reaction mechanisms and reactivity series to answer questions accurately and comprehensively.

56:28

Balancing Chemical Equations: States and Reactions

Hydrogen gas, solid Xega, and aquos states are discussed in the text.
The change in physical states from solid to gas is explained.
Displacement reactions and the release of heat are mentioned.
The evolution of gas and the importance of writing it down are highlighted.
The concept of balancing a chemical equation is introduced.
The need for balancing a chemical equation is emphasized.
The Law of Conservation of Mass is explained in relation to chemical reactions.
The importance of balancing chemical equations to respect the law is stressed.
The process of balancing a chemical equation using the hit and trial method is outlined.
Steps for writing a chemical reaction in word format and as a skeletal chemical equation are detailed.

01:16:24

Balancing Chemical Equations: Iron Oxide Addition

Iron oxide with two cations of iron is available, add it in word format.
The first chemical equation states iron plus steam gives magnetite plus hydrogen gas.
Balancing the equation is not mandatory unless you are a pro or new to chemistry.
Enclose chemical symbols in boxes to maintain the order of atoms.
Do not change the subscript of substances while balancing chemical equations.
List the number of atoms of different elements in reactants and products.
The most crucial step is to start balancing with the element having the highest number of atoms.
Balancing starts with oxygen in the equation.
Balancing involves multiplying elements to ensure equal atoms on both sides.
The balanced chemical equation follows the law of conservation of mass.

01:35:23

Chemical Reactions: States, Colors, and Catalysts

Sunil explains the transformation of solid ice into water vapor or steam, and the states of water in different forms.
Precipitators are compounds insoluble in water, forming solid precipitates after a chemical reaction.
Different compounds like barium sulphate, lead iodide, and calcium carbonate exhibit distinct colors after reactions.
The color changes in reactions, such as copper sulfide turning black, are discussed.
Concentrated and diluted acids are differentiated, with symbols used to represent them in chemical equations.
Relative terms like concentrated and diluted are explained using examples like comparing body sizes.
Heat changes in reactions are detailed, with heat being either absorbed or released during the process.
The importance of optimum conditions, including temperature, pressure, and catalysts, for maximizing product yield is emphasized.
The use of symbols like delta for heat and the representation of energy sources like electricity in reactions are explained.
The role of catalysts in increasing the speed of reactions without being consumed in the process is illustrated through a humorous analogy.

01:54:26

"Understanding Catalysts in Chemical Reactions"

A fast fight is happening with one person in the middle, discussing the benefits of fighting and the enjoyment of the public watching.
Mention of a negative catalyst named Maja Kirkira affecting the speed of reactions.
Explanation of positive and negative catalysts in chemical reactions.
Examples of positive catalysts accelerating reactions and negative catalysts slowing them down.
Emphasis on the importance of understanding catalysts in chemical reactions.
Discussion on the need for strength and positivity in facing challenges.
Explanation of combination reactions involving elements or compounds forming a single product.
Example of magnesium reacting with oxygen to form magnesium oxide, producing a white layer.
Clarification on the types of combination reactions involving elements, compounds, and elements with compounds.
Caution on the dangers of ultraviolet light emitted during reactions, leading to eye damage.

02:13:06

Chemical reactions and compound creation explained

Flying children arrive in zinc blue, potassium flame is red, sodium flame is golden yellow, and iron produces sparkles but not flame.
Lack of knowledge of CBSE is highlighted if iron does not produce flame.
Explanation of the combination of two compounds to form a compound A and A representing the compound.
The process of creating compound CD from A and B is detailed, emphasizing the compound combination reaction.
Quick lime is identified as calcium oxide, with its chemical name and common names discussed.
Reaction of calcium oxide with water to form calcium hydroxide is explained, with the chemical process detailed.
Discrepancy between NCRT and the speaker's explanation of slaked lime is discussed, emphasizing the importance of following NCRT for board exams.
The process of making slaked lime and its application as lime wash on walls is elaborated.
The reaction of calcium oxide with water to form calcium hydroxide and calcium carbonate is detailed, explaining the chemical process.
Decomposition reactions are introduced, explaining how a single compound breaks into two or more products with the input of energy like heat, electricity, or sunlight.

02:38:02

"Reactions, Industry Influence, and Safety Measures"

Energy from heat, electricity, and sunlight can cause decomposition reactions.
Reverse combination reactions can occur, resulting in multiple products from a single reactant.
In the ATC industry, Sunil Bhaya avoids sharing unpleasant truths to maintain a positive image.
Sunil Bhaya is a prominent figure in the industry, influencing many teachers and students.
The weak resort to spamming and mudslinging due to insecurity and lack of ability.
Decomposition reactions can be induced by providing energy in the form of heat, electricity, or sunlight.
Hydrated ferrous sulfate (FeSO4 7H2O) undergoes thermal decomposition when heated, releasing water and forming Fe2O3, SO2, and SO3.
Proper handling of gases released during reactions is crucial to avoid accidents and ensure safety.
Wafting gases gently towards the nose helps identify them based on their distinct smells.
The presence of sulfur dioxide and sulfur trioxide gases can be confirmed by their characteristic smells, similar to that of burning matchsticks.

02:54:40

Safety Precautions in Heating Chemical Compounds

Test tube holder is essential for safety when heating test tubes or boiling tubes to prevent burns.
Always use a test tube holder to avoid burning or injuring your hands.
CBSE 2019 question on Decomposition Reaction with Ferrous Sulfate Crystals requires precautions.
Questions in CBSE exams often relate to images or diagrams provided.
Heating calcium carbonate in a lime kiln produces calcium oxide and carbon dioxide.
Balancing chemical equations is crucial before heating compounds to ensure proper reactions.
Heating compounds can lead to the formation of multiple products.
Lead nitrate in a thermolabile tube produces brown fumes of nitrogen dioxide and oxygen gas.
Copper nitrate when heated forms black copper oxide, nitrogen dioxide, and oxygen gas.
Electrolyte decomposition involves breaking down compounds by passing electricity through them, resulting in the separation of hydrogen and oxygen gases in a 2:1 ratio.

03:13:32

Creating Electrolytes and Conducting Decomposition Reactions

Acid-laden water is created by mixing salt with water.
Electrolyte can be made at home by mixing salt in water.
Electrolyte is crucial for conducting electricity.
Dilute sulfuric acid added to water creates H+ and SO4 2- ions, enhancing conductivity.
Increasing the speed of the process requires a good conductor of electricity.
Identifying hydrogen and oxygen gases involves burning a candle near test tubes.
Hydrogen gas extinguishes a burning candle, while oxygen supports combustion.
Decomposition reactions, like that of silver chloride, occur in the presence of sunlight.
Decomposition reactions are essential in photography and require dark storage to prevent light exposure.
Decomposition reactions are generally endorsed due to the input of various forms of energy.
Reactivity in metals and non-metals determines displacement reactions, crucial in chemical reactions.

03:31:49

"Sunil's Reactivity and Displacement Reactions"

Sunil Bhaiya and Mohit Bhaiya are sitting with Radhika, with Sunil feeling more handsome and smarter.
Sunil's reactivity is highlighted, showing his superiority over others in the analogy.
The analogy extends to Sunil's interaction with Radhika and AG ji, emphasizing friendship dynamics.
Vixie Skills are introduced, involving Katrina, Salman, and Vicky Kaushal in a humorous narrative.
The reactivity series is discussed, listing metals in order of reactivity from potassium to hydrogen.
Hydrogen's unique properties as a non-metal are explained, focusing on its electron behavior.
Prateek's journey to Mathura with a car analogy is detailed, involving a humorous Punjabi exchange.
The displacement reaction concept is introduced, showcasing reactions between metals and compounds.
Specific examples of displacement reactions are provided, such as iron displacing copper and lead displacing copper.
A practical experiment involving zinc and dilute hydrochloric acid is outlined, demonstrating a displacement reaction.

03:52:05

Chemical reactions: Displacement, dissolution, and more

Displacement reactions are generally assort, and everything in the course is available for assort release.
Dissolution in water causes the temperature of substances to drop before they dissolve.
Exothermic reactions are generally the first two when water is mixed in.
Displacement reactions involve assigning Sunil.
Neutralization and gas-forming reactions will be discussed, focusing on acids, bases, and salts.
Precipitation reactions involve the formation of an insoluble solid when two ionic compounds react.
A colorless solution of lead nitrate and potassium iodide will produce yellow insoluble lead iodide.
Mixing barium hydroxide and ammonium chloride in a test tube results in a reaction that can be felt as hot or cold.
The experiment involves touching the bottom of the test tube to observe the reaction.
The reaction includes the addition of water to a piece of wood to demonstrate the reaction.

04:21:53

Freezing Reaction and Precipitation Experiments Explained

The experiment involves a beaker stuck to a wooden block, with barium hydroxide and ammonium chloride mixed inside the beaker, leading to a reaction that freezes the water between the block and beaker.
The reaction is a solid-solid double displacement reaction, with barium hydroxide and ammonium chloride reacting to absorb heat from the surroundings, causing a decrease in temperature and the formation of ice.
Another reaction is detailed involving barium chloride and sodium sulphate, resulting in the formation of barium sulphate and sodium chloride, which are insoluble solids.
The precipitation reaction between barium chloride and sodium sulphate leads to the formation of white insoluble solids, barium sulphate, and sodium chloride, with the solutions remaining colorless.
A reaction between aqueous sodium hydroxide and hydrochloric acid produces sodium chloride and water, exemplifying a double displacement reaction.

Try it yourself — It’s free.