Choose a subtopic. Topic 3: Quantitative chemistry covers Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations, Use of amount of substance in relation to masses of pure substances, Yield and atom economy of chemical reactions (chemistry only), and Using concentrations of solutions in mol/dm 3 (chemistry only) (HT only) in GCSE AQA Higher Chemistry. 23 lessons in 5 subtopics.
Revise Topic 3: Quantitative chemistry for GCSE AQA Higher Chemistry. 23 lessons across 5 subtopics.
23
Lessons
5
Subtopics
What this topic covers
Topic 3: Quantitative chemistry has 5 subtopics:
Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
Use of amount of substance in relation to masses of pure substances
Yield and atom economy of chemical reactions (chemistry only)
Using concentrations of solutions in mol/dm 3 (chemistry only) (HT only)
Use of amount of substance in relation to volumes of gases (chemistry only) (HT only)
Topic 3: Quantitative chemistry lessons by subtopic
23 lessons, grouped by subtopic.
Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
Calculating Relative Formula Mass: Learn how to calculate the relative formula mass (Mr) of compounds by adding up the relative atomic masses of all atoms in the formula, and understand how this applies to balanced chemical equations.
Percentage by Mass in Compounds: Calculate the percentage by mass of elements in compounds using relative formula mass and relative atomic masses.
Explaining Mass Changes in Open Systems: Understanding why reactions appear to involve mass changes when gases are involved, including metal oxidation and thermal decomposition examples. Learn to explain mass changes using particle models and balanced equations.
The Law of Conservation of Mass: Understand that mass is conserved in chemical reactions because no atoms are lost or made during the process, meaning the total mass of reactants equals the total mass of products.
Balancing Chemical Equations: Learn how to represent chemical reactions using balanced symbol equations, ensuring equal numbers of atoms of each element on both sides of the equation, and understand the meaning of multipliers and subscripts in chemical formulas.
Use of amount of substance in relation to masses of pure substances
Converting Masses to Moles for Equation Balancing: Learn how to convert masses in grams to amounts in moles, then use these values to determine simple whole number ratios for balancing chemical equations. Practice changing the subject of mathematical equations to solve mole calculations.
Balancing Equations from Mass Data: Apply your knowledge of mole calculations to balance chemical equations when given the masses of reactants and products. Work through step-by-step examples to convert mass data into balanced symbol equations.
Understanding Solution Concentration: Learn what concentration means in chemistry and how it is measured in terms of mass per volume (g/dm³). Understand the relationship between mass of solute, volume of solution, and concentration.
Calculating Mass of Solute in Solutions: Practice calculating the mass of solute present in a given volume of solution when you know the concentration. Apply concentration formulas to solve real-world problems.
Understanding Limiting Reactants: Learn what limiting reactants are and why they occur in chemical reactions. Understand how using an excess of one reactant ensures complete consumption of the other reactant, and identify which reactant limits the amount of products formed.
Understanding Chemical Equations in Terms of Moles: Learn how to interpret balanced chemical equations in terms of moles using the example of magnesium reacting with hydrochloric acid. Understand the relationship between coefficients and moles in equations.
Calculating Masses from Balanced Chemical Equations: Master the techniques for calculating masses of reactants and products using balanced symbol equations. Practice calculating masses when given information about one reactant or product.
Introduction to Moles and Avogadro's Constant: Learn what moles are as a unit of measurement, understand that one mole contains the same number of particles regardless of substance, and discover Avogadro's constant as the number of particles in one mole.
Yield and atom economy of chemical reactions (chemistry only)
Understanding Atom Economy: Learn what atom economy means, why it's important for sustainability and economic reasons, and understand the formula for calculating percentage atom economy from balanced equations.
Calculating and Applying Atom Economy: Practice calculating atom economy from balanced equations and explain how to choose reaction pathways based on atom economy, yield, rate and other factors.
Calculating Percentage Yield and Theoretical Mass: Master the percentage yield formula and calculation methods. Learn how to calculate theoretical mass from reactant mass and balanced equations, then determine actual percentage yields from experimental data.
Using concentrations of solutions in mol/dm 3 (chemistry only) (HT only)
Use of amount of substance in relation to volumes of gases (chemistry only) (HT only)
Gas volume fundamentals and molar volume: Learn about equal volumes of gases under same conditions and calculate gas volumes from mass using the molar volume of 24 dm³ at RTP
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Topic 3: Quantitative chemistry covers Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations, Use of amount of substance in relation to masses of pure substances, Yield and atom economy of chemical reactions (chemistry only), and Using concentrations of solutions in mol/dm 3 (chemistry only) (HT only) in GCSE AQA Higher Chemistry. 23 lessons in 5 subtopics.
What is the concentration formula?
The concentration formula is concentration = mass of solute ÷ volume of solution, measured in g/dm³. The Calculating Mass of Solute in Solutions notes cover this in full.
What is the law of conservation of mass?
The law of conservation of mass states that no atoms are lost or made during a chemical reaction, so the mass of the products equals the mass of the reactants. The The Law of Conservation of Mass notes cover this in full.
How do you calculate percentage uncertainty?
Percentage uncertainty = uncertainty ÷ measured value × 100. The Understanding Uncertainty in Chemical Measurements notes cover this in full.
What is titration?
Titration is a technique for finding an unknown concentration by reacting exact volumes of two solutions completely, with nothing left over, when the concentration of one solution is known. The Finding Unknown Concentrations Using Reaction Volumes notes cover this in full.
How do you calculate relative formula mass?
Relative formula mass (Mr) is calculated by adding up the relative atomic masses of all the atoms in a formula: multiply each element's relative atomic mass by its number of atoms, then add them together. The Calculating Relative Formula Mass notes cover this in full.
How do you balance chemical equations?
To balance a chemical equation, count the atoms of each element on both sides, then change the coefficients in front of the formulae until every element has the same number of atoms on each side. The Balancing Chemical Equations notes cover this in full.
How do you calculate percentage yield?
Percentage yield = (actual mass ÷ theoretical mass) × 100. The Calculating Percentage Yield and Theoretical Mass notes cover this in full.
What is the Mr of ethanol?
The Mr of ethanol, C₂H₅OH, is 46. The Calculating and Applying Atom Economy notes cover this in full.