Stoichiometry and Mole Calculations

70 lessons, pages 1081–1150.

  1. Stoichiometry as a Quantitative Reaction Map — From a balanced equation to testable amount predictions
  2. The Mole in Reaction Calculations — Fixed entity counts and amount of substance revisited
  3. Formula Mass and Molar Mass for Stoichiometry — Selecting the correct formula before adding atomic masses
  4. Mass–Mole Conversions in Reactions — Using n = m/M with units and reaction context
  5. Particles and Moles in a Reaction — Counting molecules, atoms and formula units with Avogadro's constant
  6. Counting Elements Inside Compound Amounts — Using subscripts to relate compound moles to atom moles
  7. Equation Coefficients as Mole Ratios — Converting balanced particle ratios into amount ratios
  8. Balance Before Calculating — Why an unbalanced equation gives false quantitative predictions
  9. Direct Mole-to-Mole Stoichiometry — Using coefficient ratios between one reactant and one product
  10. Reactant Mass to Product Moles — Mass conversion followed by a balanced mole ratio
  11. Reactant Mass to Product Mass — The complete grams–moles–moles–grams pathway
  12. Dimensional Analysis for Reaction Amounts — Writing conversion factors so units cancel visibly
  13. Precision and Significant Figures in Stoichiometry — Keeping exact coefficients separate from measured precision
  14. Atom Conservation Behind Mole Ratios — Reconciling changing molecule counts with conserved atoms
  15. Mass Conservation as a Calculation Check — Comparing total reactant and product masses in a closed system
  16. Gas Volume Ratios at Matching Conditions — Relating balanced gas coefficients to volumes at common temperature and pressure
  17. Molar Gas Volume with Stated Conditions — Using a specified volume per mole without assuming one universal value
  18. Gas Amounts from Pressure, Volume and Temperature — Introductory use of PV = nRT within a stoichiometric pathway
  19. Molarity as a Source of Reactant Moles — Using concentration times solution volume before a reaction ratio
  20. Solution Volume to Product Amount — Aqueous n = cV followed by coefficient conversion
  21. Aqueous Equation Mole Ratios — Counting dissolved species from a balanced reaction
  22. Precipitation Stoichiometry — Predicting solid product amount from soluble-ion reactants
  23. What a Limiting Reagent Means — The reactant consumed first at the balanced reaction ratio
  24. Finding the Limiting Reagent from Moles — Comparing amount divided by coefficient for each reactant
  25. Product Amount from the Limiting Reagent — Using only the reagent that caps reaction extent
  26. Excess Reagent Remaining — Subtracting reacted amount from starting amount
  27. Equal Masses Can Give Unequal Reaction Amounts — Comparing limiting behavior after converting both masses to moles
  28. Limiting Reactants in Gas Mixtures — Using volume or pressure data under specified conditions
  29. Limiting Reactants in Mixed Solutions — Concentration–volume conversion before extent comparison
  30. Three-Reactant Limiting Problems — Extending the amount-over-coefficient test to several inputs
  31. Theoretical and Actual Yield — Ideal stoichiometric maximum versus recovered product
  32. Percentage Yield Defined — Actual divided by theoretical yield times one hundred
  33. Calculating Yield from Starting Masses — Limiting reagent, theoretical mass and measured mass in one path
  34. Diagnosing an Apparent Yield Above One Hundred Percent — Wet or impure product, measurement error and formula mistakes
  35. Reactant Purity and Effective Mass — Using a purity fraction before the mole calculation
  36. Yield with an Impure Reactant — Separating sample mass from reactive substance mass
  37. Yield, Conversion and Selectivity — Keeping recovered product distinct from reactant use and side reactions
  38. Percentage Composition from a Formula — Element mass divided by compound molar mass
  39. Empirical Formula from Element Masses — Mass-to-mole conversion and smallest whole-number ratios
  40. Empirical Formula from Percentages — Choosing a hypothetical one-hundred-gram basis
  41. Converting Awkward Mole Ratios — Recognising near-half and near-third ratios without arbitrary rounding
  42. Molecular Formula from Empirical Formula Mass — Using a whole-number molar-mass multiplier
  43. Combustion Analysis of Carbon and Hydrogen — Finding C from CO2 and H from water product amounts
  44. Finding Oxygen by Mass Difference — Completing CHO empirical analysis after carbon and hydrogen
  45. Empirical Formulas of Hydrates — Comparing anhydrous-salt moles with lost-water moles
  46. Water Fraction in a Hydrated Salt — Mass-loss data and formula water count as cross-checks
  47. What an Empirical Formula Cannot Tell — Simplest ratio versus molecular identity and structure
  48. Uncertainty in Composition Data — How measurement precision affects inferred integer ratios
  49. Neutralisation Mole Ratios — Balanced acid–base equations and unequal proton counts
  50. Titration Amount Calculations — Known concentration, measured volume and reaction ratio
  51. Gas Collection and Reaction Amount — Converting a measured gas volume under stated conditions
  52. Correcting Gas-Volume Assumptions — Temperature, pressure and water-vapor cautions
  53. Redox Equations as Mole-Ratio Sources — Using a balanced redox equation without confusing electrons and moles
  54. Metal–Acid Hydrogen Calculations — Predicting H2 from metal amount and acid excess
  55. Carbonate–Acid Carbon Dioxide Calculations — Mole ratios for CO2 generation and limiting acid
  56. Decomposition and Measured Mass Loss — Inferring volatile product amount from a heated sample
  57. Atom Economy of a Balanced Reaction — Desired-product formula mass over total reactant formula mass
  58. Atom Economy Versus Percentage Yield — Reaction design metric versus experimentally recovered fraction
  59. Wet Product and Apparent Yield — Why water or impurities inflate a recovered mass
  60. Fractional Coefficients and Integer Equations — Scaling an equation without changing amount predictions
  61. Net Ionic Equations for Stoichiometry — Using reacting ion coefficients while respecting spectator ions
  62. Sequential Reaction Calculations — Carrying product moles from one balanced step into the next
  63. Overall Yield Across Several Steps — Multiplying step yields only under a consistent material-flow basis
  64. Batch Planning from a Target Product Mass — Working backward to reagent requirements
  65. Reading Stoichiometric Graphs — Slope, intercept and limiting-reagent breaks
  66. Interpreting Reaction Data Tables — Units, ratios and inconsistent observations
  67. Scaling Laboratory Equations — Moving from milligrams to kilograms without changing mole ratios
  68. Propagation of Measurement Uncertainty — Reporting sensible precision through chained calculations
  69. Mixed Stoichiometry Problem Set — Choosing between mole ratio, limiting, yield and composition methods
  70. Stoichiometry and Mole Calculations: Unit Review — Integrating balanced ratios, empirical formulas, limiting reagents and yields