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HSC Module 2 Chemistry: Introduction to Quantitative Chemsitry
1.0 Tell me more about this course
1.1 What is this course about?
1.2 How is this course different from what's on YouTube?
1.3 Worked sample problems
1.4 Downloadable Worksheets & Practice Tests
1.5 Monthly LIVE Webinars to get specific help
1.6 Graded Practice Quizes for Immediate Feddback
1.7 Linked to 'In the Lab Series' for complete understanding
1.8 Discounts for Printed Study Manuals and more
2.0 Chemical Reactions
2.1 Overview
2.2 Revision of Junior Chemical Reaction Concepts (10:19)
2.3 Balancing Chemical Equations
2.4 Common Misconceptions in Chemical Reactions
2.5 What is this thing called Stoichiometry?
2.6 How does mass change in chemical reactions?
2.7 Making Magnesium oxide in the lab (Theory)
2.8 Mass changes in liquids during a Crazy chemical change
2.9 Volume changes in chemical reactions
2.10 Investigating reaction of Zn in acid (Theory)
BONUS: Challenge- Can you get Copper out of Copper oxide?
Progress Check 1, Study Cards and Flash Card Sets
Progress Check 1 Paper
Study Cards and Flash Card Sets Sample
3.0 The Mole
3.1 Overview
3.2 What is this strange word 'the mole'?
3.3 The Mole and a person called Avogadro (4:10)
3.4 Converting between number of particles, moles and Avogadro's number (4:10)
3.5 Molar mass and usefulness in the lab (3:46)
3.6 Converting between moles, mass and formula mass
3.7 Moles and Chemical Equations (12:08)
Review of Section
4.0 Reaction Stoichiometry (Predicting using calculations)
4.1 Overview
4.2 Mole to Mole Calculations
4.3 Mole to Mass Calculations (9:37)
4.4 Mass to Mass Calculations (7:09)
4.5 Excess and Limiting Reactants
4.6 Limiting Reactant further problems (10:05)
4.7 Moles and revisiting % composition
4.8 What is meant by the term empirical formula?
4.9 Empirical formula in the lab (Theory & prac)
4.10 More challenging empirical formula questions
Section Review
5.0 Concentration of Solutions
5.1 Overview
5.2 Strong Coffee anyone? - concentration vs strength in Chemistry
5.3 Units of concentration
5.4 Concentrations in g per Litre
5.5 Concentrations in mg per Litre (or ppm)
5.6 Concentrations % by mass (%w/w)
5.7 Concentrations % by volume (%v/v)
5.8 Concentrations % by mass/volume (%w/v)
5.9 Concentrations of soutions- Moles per Litre
6.0 Molarity of Solutions
6.1 Overview
6.2 Making up a solution of known concentration (standard solution)... Theory + Prac bonus
6.3 Which solution has the greatest concentration?
6.4 Changing a concentration unit from mol / L to ppm
6.5 Dilution concept
6.6 Diluting a stock solutions to make up other solutions.
6.7 Section Review
New Lecture
7.0 Gas Reactions
71. Overview
7.2 Basics of Gas Chemistry (2:45)
7.3 What is pressure and what units does it have? (4:45)
7.4 The Gas Laws and how to remember them (5:52)
7.5 Gay-Lussac’s Law (19:02)
7.6 Boyle’s Law (6:34)
7.7 Charles’ Law (17:44)
7.8 Avogadro’s Law (3:56)
7.9 Ideal Gas Law (5:22)
11 Question Walkthroughs
11.1 Question Walkthrough Session 1 (5 questions to test your brain cells)
11.2 Question Walkthrough Session 2 (5 questions to test your brain cells)
11.3 Question Walkthrough Session 3 (5 questions to test your brain cells)
11.4 Question Walkthrough Session 4 (5 questions to test your brain cells)
11.15Question Walkthrough Session 5 (5 questions to test your brain cells)
13 Complete Learning
13.1 Learning from multiple angles
13.2 'In The LAB' Series
13.3 Professionally Printed Lab/Study Manual
13.4 Study Skills Series
13.4 Create HQ Student Materials to help learning & Earn Money
4.8 What is meant by the term empirical formula?
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