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CHAPTER 12 Gas Mixtures
18
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Page 1: Cengel ch12

CHAPTER

12

Gas Mixtures

Page 2: Cengel ch12

Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

12-1

FIGURE 12-1The mass of a mixture is equal to the sum of the masses of its components.

Page 3: Cengel ch12

Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.FIGURE 12-2The number of moles of a nonreacting mixture is equal to the sum of the number of moles of its components.

12-2

Page 4: Cengel ch12

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12-3

FIGURE 12-3The sum of the mole fractions of a mixture is equal to 1.

Page 5: Cengel ch12

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12-4

FIGURE 12-5Dalton’s law of additive pressures for a mixture of two ideal gases.

Page 6: Cengel ch12

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12-5

FIGURE 12-6Amagat’s law of additive volumes for a mixture of two ideal gases.

Page 7: Cengel ch12

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12-6

FIGURE 12-7The volume a component would occupy if it existed alone at the mixture T and P is called the component volume (for ideal gases, it is equal to the partial volume yiVm).

Page 8: Cengel ch12

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12-7

FIGURE 12-8One way of predicting the P-v-T behavior of a real-gas mixture is to use compressibility factors.

Page 9: Cengel ch12

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12-8

FIGURE 12-9Another way of predicting the P-v-T behavior of a real-gas mixture is to treat it as a pseudopure substance with critical properties Pcr and Tcr .

Page 10: Cengel ch12

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12-9

FIGURE 12-13Partial pressures (not the mixture pressure) are used in the evaluation of entropy changes of ideal-gas mixtures.

Page 11: Cengel ch12

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12-10

FIGURE 12-16It is difficult to predict the behavior of nonideal-gas mixtures because of the influence of dissimilar gas molecules on each other.

Page 12: Cengel ch12

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12-11

FIGURE 12-18For a pure substance, the chemical potential is equivalent to the Gibbs function.

Page 13: Cengel ch12

Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.FIGURE 12-20The specific volume and enthalpy of individual components do not change during mixing if they form an ideal solution (this is not the case for entropy).

12-12

Page 14: Cengel ch12

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12-13

FIGURE 12-21For a naturally occurring process during which no work is produced or consumed, the reversible work is equal to the exergy destruction.

Page 15: Cengel ch12

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12-14

FIGURE 12-22Under reversible conditions, the work consumed during separation is equal to the work produced during the reverse process of mixing.

Page 16: Cengel ch12

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12-15

FIGURE 12-23The minimum work required to separate a two-component mixture for the two limiting cases.

Page 17: Cengel ch12

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12-16

FIGURE 12-24The osmotic pressure and the osmotic rise of saline water.

Page 18: Cengel ch12

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12-17

FIGURE 12-25Power can be produced by mixing solutions of different concentrations reversibly.