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Section 14.3

Section 14.3. Ideal Gases. Ideal Gases. Solid carbon dioxide, or dry ice, doesn’t melt. It sublimes. Dry ice can exist because gases don’t obey the assumptions of kinetic theory under all conditions. You will learn how real gases differ from the ideal gases on which the gas laws are based.

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Section 14.3

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  1. Section 14.3 Ideal Gases

  2. Ideal Gases • Solid carbon dioxide, or dry ice, doesn’t melt. It sublimes. Dry ice can exist because gases don’t obey the assumptions of kinetic theory under all conditions. You will learn how real gases differ from the ideal gases on which the gas laws are based.

  3. Ideal Gas Law • Ideal Gas Law • What is needed to calculate the amount of gas in a sample at given conditions of volume, temperature, and pressure?

  4. Ideal Gas Law • To calculate the number of moles of a contained gas requires an expression that contains the variable n.

  5. Ideal Gas Law • The gas law that includes all four variables—P, V, T, and n—is called the ideal gas law. • The ideal gas constant (R) has the value 8.31 (L·kPa)/(K·mol) or 0.082 (L·atm)/(K·mol). Depending on the units of pressure, you will use one or the other.

  6. 14.5

  7. 14.5

  8. 14.5

  9. 14.5

  10. Ideal Gases and Real Gases • Ideal Gases and Real Gases • Under what conditions are real gases most likely to differ from ideal gases?

  11. Ideal Gases and Real Gases • There are attractions between the particles in an ideal gas. Because of these attractions, a gas can condense,or even solidify, when it is compressed to extremely high pressures or cooled to extremely low temperatures.

  12. Ideal Gases and Real Gases • Real gases differ most from an ideal gas at extremely low temperatures and extremely high pressures.

  13. Ideal Gases and Real Gases This graph shows how real gases deviate from the ideal gas law at extremely high pressures.

  14. The End

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