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 Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature
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