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Relative Formula Mass
Sum of relative atomic masses in a compound.
Percentage Composition
Mass percentage of an element in a compound.
Avogadro Constant
Number of particles in one mole: 6.02 x 10²³.
Mole
Amount of substance containing Avogadro's number of particles.
Mass Number
Total number of protons and neutrons in an atom.
Molar Mass
Mass of one mole of a substance in grams.
Mole Calculation Formula
Number of moles = mass (g) / Molar mass.
Conservation of Mass
Mass is neither created nor destroyed in reactions.
Balanced Equation
Equation with equal number of atoms on both sides.
Calculating % Mass
Element mass in compound / total mass x 100.
Calculating Molar Mass of Na₂CO₃
Molar mass = (2x23) + 12 + (3x16) = 106.
Mass Change
Observed mass change in unsealed reaction vessels.
Gas Reactant
Gas from air increases mass in reactions.
Gas Product
Gas formation decreases mass in reactions.
Unsealed Vessel
Allows gas escape, affecting mass measurement.
Mass Conservation
Total mass of reactants equals total mass of products.
Limiting Reactant
Reactant completely used up, stopping the reaction.
Excess Reactant
Reactant in surplus, not limiting the reaction.
Proportional Product Formation
Product amount depends on limiting reactant quantity.
Calculating Moles
Divide mass by relative formula mass (M).
Thermal Decomposition
Reaction where a compound breaks down with heat.
Gas Expansion
Gases fill available space in a container.
Molar Mass Calculation
Add atomic masses to find compound's mass.
Stoichiometry
Calculating quantities in chemical reactions.
Reactant Mass
Mass of substances before reaction starts.
Product Mass
Mass of substances formed after reaction.
Mass Loss
Occurs when gaseous products escape unsealed vessels.
Mass Gain
Occurs when gaseous reactants are consumed.
Reaction Vessel
Container where chemical reactions occur.
Moles
Unit measuring amount of substance; 1 mole = 6.022 x 10²³ particles.
Yield
Mass of product obtained from a reaction.
Theoretical Yield
Maximum mass of product calculated from reactants.
Concentration
Amount of solute per volume of solution.
Gas Volume at r.t.p.
One mole of gas occupies 24 dm³ at 20 °C.
Titration
Technique to determine concentration by neutralization.
Mass Concentration
Concentration expressed in g/dm³.
Molar Concentration
Concentration expressed in mol/dm³.
Sodium Hydroxide
Strong base used in titration to neutralize acids.
Sulfuric Acid
Strong acid commonly used in titrations.
Concentration Calculation
Formula: concentration = mass/volume.
Volume Conversion
Convert cm³ to dm³ by dividing by 1000.
Mole Calculation
Formula: moles = concentration x volume.
Uncertainty in Measurements
Variability in measurement results affecting reliability.
Gas Law
Describes behavior of gases under varying conditions.
Atom Economy
Percentage of reactants forming useful products.
Atom economy formula
Relative mass of desired products over all reactants.
100% Atom Economy
All reactants converted to useful products.
Low atom economy
High waste production in chemical reactions.
High atom economy
Efficient use of reactants with minimal waste.
Percentage Yield
Comparison of actual yield to theoretical yield.
Percentage yield formula
Actual yield divided by theoretical yield times 100.
Theoretical yield
Maximum expected product yield from a reaction.
Actual yield
Amount of product actually obtained from a reaction.
Reversible reactions
Reactions where products can revert to reactants.
Side reactions
Unintended reactions producing extra products.
Product loss during separation
Loss of material when filtering or transferring.
Neutralization reaction
Reaction between acid and base producing salt and water.
Nitric acid (HNO3)
Strong acid commonly used in titration experiments.
Mass in grams calculation
Moles multiplied by relative formula mass.
Industrial processes
Chemical reactions optimized for efficiency and yield.
Greener processes
Reactions with high atom economy and low waste.
Useful by-products
Secondary products that have economic value.
Haber process
Synthesis of ammonia from nitrogen and hydrogen.
Chemical reaction efficiency
Measure of how well reactants are converted to products.
Chemical yield
Amount of product obtained from a chemical reaction.
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