Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.
Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![4) In class, we derived the condition for equilibrium between a gas and the same chemical
dissolved in solution
Peap
Poop
YAXA
(4)
where Prap is the equilibrium pressure of the vapor, Pp, is the vapor pressure of the pure
substance, 74 is the activity coefficient of A in the solution, and XA is the mole fraction of
A in solution. We can define a constant, called the Henry's Law coefficient ka, such that
kA = PopYA. Note that ka is a property of both the chemical A (Pp) and solvent (which
determines YA). Then Equation 4 can be rewritten as
Poop = KAXA
(5)
1
Note that Equation 5 is essentially the same as Equation 4, but now it's easier to tabulate
one constant, and values of ka can be found in tables such as Table 6.1 of Tinoco. Note that
ka has units of bar, since XA is unitless (mole fraction).
Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each
gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a4dcd82-baf4-45bc-b40b-693a3e683492%2F9462cbc9-48cc-42e6-8794-60d12b297e52%2Feie2dij_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4) In class, we derived the condition for equilibrium between a gas and the same chemical
dissolved in solution
Peap
Poop
YAXA
(4)
where Prap is the equilibrium pressure of the vapor, Pp, is the vapor pressure of the pure
substance, 74 is the activity coefficient of A in the solution, and XA is the mole fraction of
A in solution. We can define a constant, called the Henry's Law coefficient ka, such that
kA = PopYA. Note that ka is a property of both the chemical A (Pp) and solvent (which
determines YA). Then Equation 4 can be rewritten as
Poop = KAXA
(5)
1
Note that Equation 5 is essentially the same as Equation 4, but now it's easier to tabulate
one constant, and values of ka can be found in tables such as Table 6.1 of Tinoco. Note that
ka has units of bar, since XA is unitless (mole fraction).
Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each
gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.
![He is the least soluble, and C,H, and CO, are the most soluble. Gas solubility is also a
gases,
function of temperature and depends on the solvent. Oxygen is about 20% less soluble at 37°C
(physiological temperature) than at 25°C. Note that lower numbers mean higher solubility.
TABLE 6 Henry's Law coefficients kg = Py.p/xg, in bar, for aqueous solutions
Gas
O°C
25°C
37°C
He
131 x 103
139 X 10
138 X 10
50X 103
84 x 10
98 X 103
CO
35X 10
57 x 103
67x 10
26 X 10
42 x 10
50x 10
0,
CH,
23 X 10
38X 10
46 x 10
Ar
24 x 10
38X 10
45 X 10
CO2
0.71 X 10
1.59X 10
2.13 x 10
CH,
0.71 X 10
1.32 X 10
1.69 X-10
Source: Based on data from Harvey, A. H. "Semiempirical correlation for Henry's constants over large temperature ranges."
AICHE Journal, 42, pp. 1491 1494. DOL 101002/aic.690420531. Copyright (c) 1966 John Wiley and Sons, Inc.
Phase Equilibria205](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a4dcd82-baf4-45bc-b40b-693a3e683492%2F9462cbc9-48cc-42e6-8794-60d12b297e52%2F7su9x6q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:He is the least soluble, and C,H, and CO, are the most soluble. Gas solubility is also a
gases,
function of temperature and depends on the solvent. Oxygen is about 20% less soluble at 37°C
(physiological temperature) than at 25°C. Note that lower numbers mean higher solubility.
TABLE 6 Henry's Law coefficients kg = Py.p/xg, in bar, for aqueous solutions
Gas
O°C
25°C
37°C
He
131 x 103
139 X 10
138 X 10
50X 103
84 x 10
98 X 103
CO
35X 10
57 x 103
67x 10
26 X 10
42 x 10
50x 10
0,
CH,
23 X 10
38X 10
46 x 10
Ar
24 x 10
38X 10
45 X 10
CO2
0.71 X 10
1.59X 10
2.13 x 10
CH,
0.71 X 10
1.32 X 10
1.69 X-10
Source: Based on data from Harvey, A. H. "Semiempirical correlation for Henry's constants over large temperature ranges."
AICHE Journal, 42, pp. 1491 1494. DOL 101002/aic.690420531. Copyright (c) 1966 John Wiley and Sons, Inc.
Phase Equilibria205
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