1. Zumdahl Zumdahl DeCoste
World of
CHEMISTRY

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Chapter 13
Gases
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Figure 13.2: A glass tube is filled with mercury and inverted in a dish of mercury at sea level.
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4. Figure 13.3: Gas pressure = atmospheric pressure – h.
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5. Figure 13.3: Gas pressure = atmospheric pressure + h.
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Table 13.1
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7. Figure 13.4: A J-tube similar to the one used by Boyle.
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8. Figure 13.5: A plot of P versus V from Boyle’s data.
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9. Figure 13.6: Illustration of Boyle’s law.
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10. Figure 13.7: Plots of V (L) versus T (°C) for several gases.
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Figure 13.8: Plots of V versus T using the Kelvin scale for temperature.
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12. Figure 13.9: The relationship between volume V and number of moles n.
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Figure 13.10: When two gases are present, the total pressure is the sum of the partial pressures of the gases.
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Figure 13.11: The total pressure of a mixture of gases depends on the number of moles of gas particles present.
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15. Figure 13.12: The production of oxygen by thermal decomposition.
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Postulates of KMT.
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Figure 13.13: (a) A gas confined in a cylinder with a movable piston (b) The temperature of the gas is increased at constant pressure P ext..
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18. Figure 13.14: A gas sample is compressed.
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