20 Relationship between Pressure & Temperature of Gases P-T
21 In mathematical terms: y = mx + bP = mT + bGay-Lussac’s Law
22 Relationship between Volume & Moles of GasesV-n
23 In mathematical terms: y = mx + bV = mn + bAvogadro’s Law
24 Avogadro’s Hypothesis At constant temperature and pressure, equal volumes of gases contain equal number of particles
25 3. Hydrogen gas [8. 3 liters] reacts in the presence of 2 3. Hydrogen gas [8.3 liters] reacts in the presence of 2.5 liters of nitrogen gas at 370C and 100 kPa. What volume of ammonia is produced at these same conditions?
28 Kinetic Molecular Theory 1. Gases consist of small particles that are far apart in comparison to their own size. These particles are considered to be tiny points occupying a negligible volume compared to that of their container.
29 Kinetic Molecular Theory 2. Molecules are in rapid and random straight-line motion. This motion can be described by well-defined and established laws of motion.
30 Kinetic Molecular Theory 3. The collisions of molecules with the walls of a container or with other molecules are perfectly elastic. That is, no loss of energy occurs.
31 Kinetic Molecular Theory 4. There are no attractive forces between molecules or between molecules and the walls with which they collide.
32 Kinetic Molecular Theory 5. At any particular instant, the molecules in a given sample of gas do not all possess the same amount of energy.
33 PARTICLEIN THEBOXHave 1 particle,with mass m,with velocity