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Chapter 8 - Gases

8.1 - Properties of Gases

  • In a gas, particles are so distant and moving that their attractions are insignificant.

    • The physical characteristics of pressure (P), volume (V), temperature (T), and quantity in moles describe gas (n)

  • A gas exerts pressure, the strength of the gas particles hitting the container surface’

    • Units like torr, mmHg, atm, and Pa measure the gas pressure

8.2 - Pressure and Volume (Boyle’s Law)

  • If there is no change in temperature and quantity of gas, the volume (V) of a gas changes inversely with the gas pressure (P).

    • When the volume decreases, the pressure increases and decreases as the volume increases.

8.3 - Temperature and Volume (Charles’s Law)

  • When there is no change in pressure and gas volume, the (V) volume of a gas is directly related to its kelvin temperature (T).

    • Increasing the temperature of a gas will increase the volume while decreasing the temperature, volume.

8.4 - Temperature and Pressure (Gay-Lussac’s Law)

  • If no change is made in volume and gas quantity, the pressure (P) of the gas is directly related to its Kelvin (T) temperature.

    • With increasing gas temperature, its pressure increases; if the temperature drops, the pressure falls.

8.5 - The Combined Gas Law

  • When the quantity is not changed, the combined gas law is the relationship between pressure (P), volume (V), and temperature (T).

  • The combined gas law shall be used to assess the effect of change on the third in two of the variables.

8.6 - Volume and Moles (Avogadro’s Law)

  • The volume (V) of a gas is directly related to the number of moles (n) of the gas when the pressure and temperature of the gas do not change.

  • Increasing the volume of the gas moles; decreasing the gas moles must decrease the volume.

    • 1 mole of any gas has a volume of 22.4 L at Standard Temperature (273 K) and Standard Pressure (1 atm), STP abbreviated.

8.7 - Partial Pressures (Dalton’s Law)

  • The total is a combination of two or more gasses is the total of partial pressures of every single gas.

    • The pressure of the partial gas in a mixture is the pressure it would exert if the gas in the container was the only gas.

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8.1 - Properties of Gases

  • In a gas, particles are so distant and moving that their attractions are insignificant.

    • The physical characteristics of pressure (P), volume (V), temperature (T), and quantity in moles describe gas (n)

  • A gas exerts pressure, the strength of the gas particles hitting the container surface’

    • Units like torr, mmHg, atm, and Pa measure the gas pressure

8.2 - Pressure and Volume (Boyle’s Law)

  • If there is no change in temperature and quantity of gas, the volume (V) of a gas changes inversely with the gas pressure (P).

    • When the volume decreases, the pressure increases and decreases as the volume increases.

8.3 - Temperature and Volume (Charles’s Law)

  • When there is no change in pressure and gas volume, the (V) volume of a gas is directly related to its kelvin temperature (T).

    • Increasing the temperature of a gas will increase the volume while decreasing the temperature, volume.

8.4 - Temperature and Pressure (Gay-Lussac’s Law)

  • If no change is made in volume and gas quantity, the pressure (P) of the gas is directly related to its Kelvin (T) temperature.

    • With increasing gas temperature, its pressure increases; if the temperature drops, the pressure falls.

8.5 - The Combined Gas Law

  • When the quantity is not changed, the combined gas law is the relationship between pressure (P), volume (V), and temperature (T).

  • The combined gas law shall be used to assess the effect of change on the third in two of the variables.

8.6 - Volume and Moles (Avogadro’s Law)

  • The volume (V) of a gas is directly related to the number of moles (n) of the gas when the pressure and temperature of the gas do not change.

  • Increasing the volume of the gas moles; decreasing the gas moles must decrease the volume.

    • 1 mole of any gas has a volume of 22.4 L at Standard Temperature (273 K) and Standard Pressure (1 atm), STP abbreviated.

8.7 - Partial Pressures (Dalton’s Law)

  • The total is a combination of two or more gasses is the total of partial pressures of every single gas.

    • The pressure of the partial gas in a mixture is the pressure it would exert if the gas in the container was the only gas.

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