Unit 9

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Across
  1. 6. Conversion The process of converting between moles of different substances using mole ratios from a balanced chemical equation.
  2. 11. Particles The smallest units of a substance, such as atoms, molecules, or formula units, that retain the substance's properties.
  3. 12. Coefficients The numbers in a balanced chemical equation that indicate the proportions of reactants and products in a reaction.
  4. 13. Ratio The ratio of moles of one substance to moles of another in a balanced chemical equation.
  5. 14. of Definite Proportions A principle stating that a given chemical compound always contains its component elements in fixed ratios by mass.
  6. 15. Reactant The reactant that is completely consumed in a chemical reaction, determining the maximum amount of product that can be formed.
  7. 17. Gas Law The equation PV = nRT, which describes the behavior of an ideal gas.
  8. 18. to Moles Conversion The process of converting mass (grams) to moles.
  9. 20. Number The number of particles (6.022 × 10²³) in one mole of a substance.
Down
  1. 1. The amount of solute present in a given quantity of solvent or solution, often expressed in molarity (moles per liter).
  2. 2. A form of matter that has a constant chemical composition and distinct properties, either an element or a compound.
  3. 3. Formula The simplest whole-number ratio of atoms of each element in a compound.
  4. 4. A unit of measurement in chemistry representing 6.022 × 10²³ particles (atoms, molecules, or ions) of a substance.
  5. 5. Analysis A mathematical technique used to convert units by using conversion factors based on relationships between units.
  6. 7. Reaction A process in which substances (reactants) undergo chemical changes to form new substances (products).
  7. 8. The quantitative relationship between reactants and products in a chemical reaction, based on balanced chemical equations.
  8. 9. Volume The volume occupied by one mole of a gas at standard temperature and pressure (STP), which is approximately 22.4 liters for an ideal gas.
  9. 10. Composition The percentage by mass of each element in a compound.
  10. 16. Formula The actual number of atoms of each element in a molecule of a compound, which may be a multiple of the empirical formula.
  11. 19. Mass The mass of one mole of a substance, expressed in grams per mole (g/mol), equivalent to the sum of the atomic masses of its constituent atoms.