13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature We have developed macroscopic definitions of pressure and temperature. Pressure is the force divided by the area on which the force is exerted, and temperature is measured with a thermometer. We gain a better understanding of pressure and temperature from the kinetic theory of gases, which assumes that atoms and molecules are in continuous random motion. Figure 13.20 When a molecule collides with a rigid wall, the component of its momentum perpendicular to the wall is reversed. A force is thus exerted on the wall, creating pressure.
13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature We have developed macroscopic definitions of pressure and temperature. Pressure is the force divided by the area on which the force is exerted, and temperature is measured with a thermometer. We gain a better understanding of pressure and temperature from the kinetic theory of gases, which assumes that atoms and molecules are in continuous random motion. Figure 13.20 When a molecule collides with a rigid wall, the component of its momentum perpendicular to the wall is reversed. A force is thus exerted on the wall, creating pressure.
13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature We have developed macroscopic definitions of pressure and temperature. Pressure is the force divided by the area on which the force is exerted, and temperature is measured with a thermometer. We gain a better understanding of pressure and temperature from the kinetic theory of gases, which assumes that atoms and molecules are in continuous random motion. Figure 13.20 When a molecule collides with a rigid wall, the component of its momentum perpendicular to the wall is reversed. A force is thus exerted on the wall, creating pressure.
Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature • Express the ideal gas law in terms of molecular mass and velocity. • Define thermal energy. • Calculate the kinetic energy of a gas molecule, given its temperature. • Describe the relationship between the temperature of a gas and the kinetic energy of atoms and molecules. • Describe the distribution of speeds of molecules in a gas.
Transcribed Image Text:13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and
Temperature
We have developed macroscopic definitions of pressure and temperature. Pressure is the force divided by the area on which the
force is exerted, and temperature is measured with a thermometer. We gain a better understanding of pressure and temperature
from the kinetic theory of gases, which assumes that atoms and molecules are in continuous random motion.
Figure 13.20 When a molecule collides with a rigid wall, the component of its momentum perpendicular to the wall is reversed. A force is thus exerted
on the wall, creating pressure.
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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