d Metal Data 22242 Trial 1 Trial 2 1 Mass of Magnesium (g) G620 G034 2. Volume of Hydrogen Gas Collected (mL) 22 2 3. Temperature (C) 22.2 225 205 35 29563 4. Temperature K) (show calculation) 5. Barometric Pressure (mm Hg) Height Difference between Water Levels 6. 2A0 910 (mm H,O) Mercury Equivalent of Height Difference Water Difference 7. (show calculation) 13.6 Vapor Pressure of Water 8 (will be given-mm Hgl 19.8 Pressure of Dry Hydrogen Gas Barometric Pressure - Mercury Equivalent 9. of Height Difference - Vapor Pressure of Water (show calculation) Number of Mole of Hydrogen Gas Collected 10. Number of Mole of Metal 11. Molar Mass of a Solid (g/mo) 12. Average Molar Mass 13.

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Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.