Molecular Physics

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)

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)