06CHEM20: Chapter 3 - Stoichiometry | IGCSE Chemistry | Prof Pras

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Published on March 8, 2025 4:35:33 AM ● Video Link: https://www.youtube.com/watch?v=c7-N3cq4u-I

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06CHEM20: Chapter 3 - Stoichiometry | IGCSE Chemistry | Prof Pras
📢 Welcome back to our IGCSE Chemistry series! In this lesson, we dive deep into Stoichiometry, one of the most important topics in Chemistry. Whether you're preparing for your IGCSE exams or just want to master chemical calculations, this lesson will break it down in a simple and engaging way. 🧪✨

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🌟 What You’ll Learn in This Video:
✅ What is Stoichiometry? Understanding the mole concept and balanced chemical equations
✅ Relative Atomic Mass (Ar) & Relative Molecular Mass (Mr) – How to calculate them
✅ The Mole Concept & Avogadro’s Constant (6.022 × 10²³)
✅ Molar Ratios & Chemical Equations – Understanding reactants & products
✅ Limiting Reactants & Excess Reactants – How to determine them
✅ Percentage Yield & Percentage Purity – Real-life applications in Chemistry
✅ Empirical & Molecular Formula – Understanding their differences

🤔 Why Watch This Video?
🔬 Clear & Simple Explanations – Learn Chemistry with visual animations and real-world examples.
📖 Exam-Focused Content – We cover everything you need for IGCSE Chemistry exams.
🧠 Stronger Understanding – Build a solid foundation in chemical calculations.
🔥 Perfect for Quick Revision – Recap key points before your exam!

🎯 Who is this video for?
✅ IGCSE & GCSE Chemistry students
✅ O-Level Chemistry students
✅ Anyone struggling with Stoichiometry & Moles
✅ Science enthusiasts who want to master Chemistry

📝 Quick Notes: Key Points from the Lesson
1️⃣ What is Stoichiometry?
The study of quantitative relationships in a chemical reaction.
Helps us determine how much reactant is needed or how much product is formed.
2️⃣ The Mole Concept & Avogadro’s Constant
1 mole = 6.022 × 10²³ particles (atoms, molecules, or ions).
Molar Mass = Mass of 1 mole of a substance (g/mol).
3️⃣ Relative Atomic Mass (Ar) & Molecular Mass (Mr)
Ar = The average mass of an atom compared to carbon-12.
Mr = The sum of all atomic masses in a molecule.
4️⃣ Balancing Chemical Equations
Ensuring that the number of atoms of each element is equal on both sides.
Example: 2H₂ + O₂ → 2H₂O
5️⃣ Molar Ratios & Chemical Reactions
The ratio of reactants to products in a balanced equation.
Example: 2H₂ + O₂ → 2H₂O means 2 moles of hydrogen react with 1 mole of oxygen to form 2 moles of water.
6️⃣ Limiting & Excess Reactants
Limiting Reactant: The reactant that gets used up first, stopping the reaction.
Excess Reactant: The reactant left over after the reaction is complete.
7️⃣ Percentage Yield & Percentage Purity
Percentage Yield = (Actual Yield / Theoretical Yield) × 100
Percentage Purity = (Pure Substance / Total Sample) × 100
8️⃣ Empirical & Molecular Formula
Empirical Formula: The simplest whole-number ratio of atoms in a compound.
Molecular Formula: The actual number of atoms in a molecule.

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