Across
- 2. The number of atoms, ions, or molecules in one mole of a substance. (2 words)
- 5. The quantity of a substance that contains the same number of entities (atoms, molecules, or particles)(3 words)
- 6. A combination of all gas laws. (3 words)
- 8. Assumption that gas molecules do not exert attractive or repulsive forces on each other, meaning their interactions are limited to elastic collisions. (3 words)
- 10. Assumption that when gas molecules collide with each other or the container walls, they do not lose kinetic energy, meaning total energy is conserved. (2 words)
- 13. The total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. (5 words)
- 14. Law At constant volume, the pressure of a gas is directly proportional to its absolute temperature. (3 words)
- 15. A theoretical gas that follows the equation PV=nRT under all conditions, assuming no intermolecular interactions and that gas molecules occupy negligible volume. (2 words)
- 16. The mass of one mole of a given substance, expressed in grams per mole (g/mol). (2 words)
Down
- 1. Assumption that gas molecules are so small compared to the volume of the container that their own volume is negligible. (2 words)
- 3. At constant temperature, the pressure of a gas is inversely proportional to its volume. (2 words)
- 4. The constant relating the average kinetic energy of particles in a gas to the temperature. It is the gas constant divided by Avogadro’s number. (2 words)
- 7. The total count of individual molecules present in a given amount of substance. (3 words)
- 9. A physical constant used in the ideal gas law, representing the relationship between energy, temperature, and moles of a gas. (3 words)
- 11. At constant pressure, the volume of a gas is directly proportional to its absolute temperature. (2 words)
- 12. Assumption that gas molecules move in completely random directions with varying speeds. (2 words)