Mole Concept || Atoms and Molecules - 12 || in Hindi for Class 9 Science NCERT

EduPoint Class 9 & 10

13 Aug 202028:47

EducationalLearning

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TLDRThe video script discusses the concept of moles in chemistry, relating it to everyday examples like buying fruits and vegetables by weight. It explains the mole as a unit to measure the amount of substance, introducing Avogadro's number as a significant figure in chemical reactions. The script clarifies the difference between atomic mass, molecular mass, and molar mass, using examples like hydrogen, carbon, and oxygen to illustrate calculations. It also covers the importance of understanding moles for chemical equations and reactions, such as the formation of water from hydrogen and oxygen.

Takeaways

😀 The video discusses the concept of moles in the context of chemistry, specifically from the 'Standard Ninth Chemistry' textbook's chapter on 'Items and Objectives'.
📚 It explains the relationship between relative atomic mass, molar mass, and how these concepts connect to everyday life, such as market rates and purchasing by weight.
🍇 The video uses the example of buying fruits like grapes to illustrate the concept of molar mass and how it applies to the number of particles in a given mass.
🔢 It introduces Avogadro's number (6.02 × 10^23) as a fundamental constant in chemistry, which represents the number of particles in one mole of a substance.
🌍 The video clarifies the concept of molar mass, explaining it as the mass of one mole of a substance, and how it is used to calculate the mass of atoms and molecules.
🧪 The script explores the atomic mass of elements like hydrogen, carbon, and oxygen, and how to calculate the molar mass of molecules such as carbon dioxide (CO2) and water (H2O).
🔗 It emphasizes the importance of understanding the difference between atomic mass and molar mass, and how these concepts are used in chemical reactions.
🧩 The video provides examples of how to calculate the number of moles in a sample and how to convert between grams and moles using molar mass.
📉 The transcript mentions the use of formulas to determine the number of molecules in a sample and how to represent chemical reactions with equations.
💡 It highlights the significance of Avogadro's number in stoichiometry, which is used to find out how many particles are in a mole of a substance.
🔄 The video script also touches on the concept of doubling or tripling samples in chemical reactions and how it affects the number of molecules and moles.

Q & A

What is the topic of the video?
-The video discusses the concept of moles in chemistry, specifically from the chapter 'Items and Objectives' of Standard Ninth Chemistry.
What is the significance of the term 'mole' in chemistry?
-In chemistry, a 'mole' is a unit that represents the amount of a chemical substance, and it is used to count the number of atoms, molecules, or ions in a sample.
What is the Avogadro's number, and how is it used in chemistry?
-Avogadro's number is approximately 6.02 × 10^23, and it represents the number of particles (atoms, molecules, ions, etc.) in one mole of a substance.
How is the atomic mass related to the mass of a mole of atoms?
-The atomic mass of an element, expressed in atomic mass units (amu), when multiplied by Avogadro's number, gives the mass of one mole of that element in grams.
What is the difference between relative atomic mass and actual mass?
-The relative atomic mass is a dimensionless quantity (the number 1) that indicates how much one atom of an element weighs relative to 1/12th the mass of a carbon-12 atom. The actual mass, on the other hand, is the mass of an atom expressed in grams.
Can you explain the concept of molar mass?
-Molar mass is the mass of one mole of a substance. It is calculated by multiplying the atomic mass of an element (in atomic mass units) by Avogadro's number, resulting in the mass of one mole of that element in grams.
What is the molar mass of hydrogen atoms?
-The atomic mass of a hydrogen atom is approximately 1 amu. Therefore, the molar mass of hydrogen is about 1 gram per mole, since 1 mole of hydrogen atoms contains Avogadro's number of hydrogen atoms.
How is the mass of a mole of molecules calculated?
-The mass of a mole of molecules is calculated by multiplying the molecular mass (the sum of the atomic masses of all atoms in a molecule) by Avogadro's number.
What is the molar mass of carbon dioxide (CO2)?
-The molar mass of carbon dioxide is calculated by adding the atomic mass of one carbon atom (approximately 12 amu) and twice the atomic mass of one oxygen atom (approximately 16 amu each), resulting in a molar mass of about 44 grams per mole.
What is the significance of Avogadro's number in stoichiometry?
-Avogadro's number is crucial in stoichiometry because it allows chemists to convert between the amount of substance in moles and the number of individual particles (atoms, molecules, ions) in a sample.
How does the video explain the concept of molecular mass?
-The video explains molecular mass by describing it as the sum of the atomic masses of all atoms within a molecule, and it shows how to calculate the mass of a mole of a particular molecule.

Outlines

00:00

🔬 विज्ञान के मॉल कॉन्सेप्ट का परिचय

इस खंड में वीडियो स्क्रिप्ट ने विज्ञान के मॉल कॉन्सेप्ट पर चर्चा की है। यह स्टैंडर्ड नाइंथ केमिस्ट्री के चैप्टर 'आइटम्स एंड ऑब्जेक्टिव्स' का हिस्सा है। वीडियो में मॉल के साथ संबंधित विभिन्न अवधारणाएँ, जैसे कि रिलेटिव एटॉमिक मास, ग्राम एटॉमिक मास, मॉलिक्यूलर मास, ग्राम मॉलिक्यूलर मास और मॉल की चीज़ें पर विस्तृत चर्चा की गई है। यहाँ पर मॉल के रूप में एक बड़ी संख्या, जो कि 6.02 * 10^23 सेट को दर्ज़ करती है, का परिचय किया गया है जो कि क्लेयर होगा जैसे कि किमिकल रिएक्शन में मॉलिक्यूल पार्टिसिपेट करता है।

05:02

🧪 एटॉमिक और मॉलिक्यूलर मास के बीच के संबंध

इस खंड में, एटॉमिक और मॉलिक्यूलर मास के बीच के संबंध और उनके उपयोग के बारे में चर्चा की गई है। यहाँ पर विषय के लिए उदाहरण दिए गए हैं, जैसे कि हाइड्रोजन, कार्बन और हीलियम के एटॉमिक मास के बारे में बात की गई है और कैसे उनका ग्राम एटॉमिक मास निर्धारित किया जा सकता है। इसके अतिरिक्त, विषय के लिए आइसोटोप्स और उनके टॉमिक मास के बारे में भी चर्चा की गई है, जिसमें कार्बन के विभिन्न आइसोटोप्स के बारे में जानकारी प्रदान की गई है।

10:03

📚 मॉलिक्यूलर मास और विज्ञान के अवधारणाओं का अध्ययन

इस खंड में, मॉलिक्यूलर मास के अवधारणा और विज्ञान के अन्य महत्वपूर्ण अवधारणाओं को विस्तार से अध्ययन किया गया है। यहाँ पर मॉलिक्यूलर मास के बारे में विस्तृत चर्चा की गई है, जिसमें मॉलिक्यूल के मांस की गणना और मॉलिक्यूलर मास की महत्वत्ता पर जोर दिया गया है। इसके अतिरिक्त, मॉलिक्यूलर मास के साथ संबंधित अवधारणाओं को समझाने के लिए उदाहरण दिए गए हैं, जैसे कि हाइड्रोजन और ऑक्सीजन के मॉलिक्यूल के मांस का विश्लेषण।

15:03

🔍 हीलियम, कार्बन डायऑक्साइड और नाइट्रोजन के मॉलिक्यूलर मास का विश्लेषण

इस खंड में, हीलियम, कार्बन डायऑक्साइड और नाइट्रोजन के मॉलिक्यूलर मास के बारे में विस्तृत चर्चा की गई है। यहाँ पर हीलियम के मॉनोएटॉमिक मॉलिक्यूलर फॉर्म के बारे में बात की गई है, और कैसे इसे मॉलिक्यूल के रूप में दर्शाया जा सकता है। इसके अतिरिक्त, कार्बन डायऑक्साइड और नाइट्रोजन के मॉलिक्यूलर मास के बारे में विस्तृत जानकारी प्रदान की गई है, जिसमें उनके ग्राम मॉलिक्यूलर मास और रिलेटिव मॉलिक्यूलर मास के बारे में चर्चा की गई है।

20:04

📈 कार्बन डायऑक्साइड के सैंपल के मॉलिक्यूलर गणना

इस खंड में, कार्बन डायऑक्साइड के सैंपल के मॉलिक्यूलर गणना के बारे में चर्चा की गई है। यहाँ पर एक सैंपल में कार्बन डायऑक्साइड के मॉलिक्यूल्स की संख्या की गणना करने के लिए एक फॉर्मूला का उपयोग किया गया है। यहाँ पर ग्राम मॉलिक्यूलर मास के आधार पर मॉलिक्यूल्स की संख्या का निर्धारण करने के लिए विस्तृत चरणों का विवरण दिया गया है।

25:06

🧐 हाइड्रोजन और ऑक्सीजन के रिएक्शन का मॉलिक्यूलर विश्लेषण

इस खंड में, हाइड्रोजन और ऑक्सीजन के रिएक्शन का मॉलिक्यूलर विश्लेषण किया गया है। यहाँ पर एक सैंपल के मॉलिक्यूलर स्तर पर रिएक्शन के बारे में चर्चा की गई है, जिसमें हाइड्रोजन और ऑक्सीजन के मॉलिक्यूल्स के संख्या को डबल करने का परिणाम और उसने कितने वाटर मॉलिक्यूल्स का निर्माण किया है, इसका विश्लेषण किया गया है। इसके अतिरिक्त, रिएक्शन के संबंध में मॉलिक्यूलर मास और मॉल की संख्या के महत्व के बारे में भी चर्चा की गई है।

🔍 मॉलिक्यूलर गणना और रिएक्शन के परिणाम का विश्लेषण

इस खंड में, मॉलिक्यूलर गणना और रिएक्शन के परिणाम का विश्लेषण किया गया है। यहाँ पर मॉलिक्यूलर स्तर पर रिएक्शन के परिणामों का विश्लेषण किया गया है, जिसमें हाइड्रोजन, ऑक्सीजन और वाटर के मॉलिक्यूल्स के संख्या को निर्धारण करने के लिए विस्तृत चर्चा की गई है। इसके अतिरिक्त, रिएक्शन के परिणामों को समझने के लिए मॉलिक्यूलर मास और मॉल की संख्या का महत्व विस्तार से समझाया गया है।

Mindmap

Keywords

💡Molar Concept

The molar concept refers to the amount of a substance measured in moles, where one mole contains Avogadro's number of particles, approximately 6.02×10^23. In the video, this concept is central to understanding chemical reactions and the relationships between mass, atomic mass, and molecular mass. For example, when discussing the mass of hydrogen atoms and molecules, the molar concept helps to calculate the total mass of a large number of particles.

💡Atomic Mass

Atomic mass is the mass of a single atom, typically measured in atomic mass units (amu). It is a fundamental concept in the video, as it helps to determine the mass of elements in a compound. For instance, the script mentions the atomic mass of hydrogen (1 amu) and carbon (12 amu), which is used to calculate the molar mass of molecules like carbon dioxide (CO2).

💡Molecular Mass

Molecular mass is the total mass of all the atoms in a molecule, and it is calculated by adding the atomic masses of the constituent atoms. The video explains how to determine the molecular mass of various molecules, such as water (H2O) and carbon dioxide (CO2), using the atomic masses of the individual elements that make up the molecules.

💡Avogadro's Number

Avogadro's number, approximately 6.02×10^23, is the number of constituent particles (usually atoms or molecules) in one mole of a substance. The video emphasizes its importance in chemistry for quantifying the relationships between moles, atoms, and molecules. It is used to establish the equivalence between molar mass and mass in grams.

💡Gram Atomic Mass

Gram atomic mass is the mass of one mole of atoms of an element, measured in grams. The video script uses this concept to explain how many atoms are present in a certain mass of an element, such as hydrogen or carbon, by relating it to the atomic mass and Avogadro's number.

💡Gram Molecular Mass

Gram molecular mass is the mass of one mole of a molecule, also measured in grams. The video discusses how to calculate the total mass of a mole of a specific molecule by multiplying the molecular mass by Avogadro's number and converting it to grams.

💡Relative Atomic Mass

Relative atomic mass is a dimensionless value that compares the mass of an atom to a defined standard, usually carbon-12, which is assigned a relative atomic mass of 12. The video script uses this concept to simplify calculations and comparisons of atomic masses between different elements.

💡Isotopes

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. The video mentions carbon isotopes, such as carbon-12 and carbon-14, to illustrate variations in atomic mass within the same element.

💡Chemical Reactions

Chemical reactions involve the rearrangement of atoms to form new substances. The video script provides an example of a chemical reaction between hydrogen and oxygen to form water, highlighting the conservation of mass and the role of molar quantities in balancing chemical equations.

💡Mole Calculations

Mole calculations are used to determine the number of moles of a substance, which is essential for understanding the proportions in which reactants and products are involved in chemical reactions. The video demonstrates how to use the molar mass and the mass of a substance to calculate the number of moles, as seen when discussing the molar mass of carbon dioxide and its sample mass.

💡Molar Ratios

Molar ratios are used to express the relationship between the amounts of different substances in a chemical reaction, ensuring that the law of conservation of mass is upheld. The video explains how to use molar ratios to balance chemical equations, such as the reaction between hydrogen and oxygen to produce water.

Highlights

Discussion on molar concept in chemistry, relating to Standard Ninth Chemistry's chapter on items and objectives.

Explanation of the term 'mole' in the context of chemistry, and its significance in measuring chemical substances.

Differentiating between relative atomic mass, actual atomic mass, and molar mass.

The concept of Avogadro's number and its role in understanding the quantity of molecules in a mole.

How to calculate the mass of atoms and molecules using the mole concept.

The importance of molar mass in chemical reactions and calculations.

Understanding the mole concept in terms of atomic and molecular masses.

The relationship between molar mass and the amount of substance in grams.

Conversion between grams and moles using Avogadro's number.

Explanation of atomic mass unit (amu) and its equivalence to grams.

Calculating the molar mass of elements like hydrogen, carbon, and oxygen.

Understanding the molar mass of compounds such as carbon dioxide (CO2).

The significance of molar mass in stoichiometry and balancing chemical equations.

How to determine the number of molecules in a given mass of a substance.

Practical applications of molar mass in everyday life, such as buying goods by weight.

The use of molar mass to solve numerical problems in chemistry.

Connecting the mole concept to real-world scenarios, like buying fruits by weight and understanding the rate per kilogram.

The role of molar mass in understanding the composition of molecules and compounds.

Summary of the key points discussed in the video, emphasizing the importance of molar mass in chemistry.

Transcripts

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Related Tags

Chemistry Basics Molar Concept Atomic Mass Avogadro's Number Molecular Mass Chemical Reactions Educational Content Science Learning Molecular Science Numerical Problems