11: Chapter 9 - Gases
- Page ID
- 369583
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- 11.1: Pressure and units
- The kinetic theory of gases indicates that gas particles are always in motion and are colliding with other particles and the walls of the container holding them. Although collisions with container walls are elastic (i.e., there is no net energy gain or loss because of the collision), a gas particle does exert a force on the wall during the collision. The accumulation of all these forces, distributed over the area of the walls of the container, causes pressure.
- 11.2: Combined gas law
- The combined gas law expresses the relationship between the pressure, volume, and absolute temperature of a fixed amount of gas. For a combined gas law problem, only the amount of gas is held constant.
- 11.3: Ideal Gas Law
- The ideal gas law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas.
- 11.4: Partial pressure
- The partial pressure of a gas is the contribution that gas makes to the total pressure when the gas is part of a mixture. Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of all of the partial pressures of the component gases.
- 11.5: Gas collection by water displacement
- Gases that are produced in laboratory experiments are often collected by a technique called water displacement. Because the gas is collected over water, it is not pure, but is mixed with vapor from the evaporation of the water. Dalton's law can be used to calculate the amount of the desired gas by subtracting the contribution of the water vapor.