A particular gas has a solubility in water of 1.75 mM when the pressure of the gas above water is 0.625 atm. What must the pressure of the pressure (in atm) of the gas above water be in order for the solubility to be 4.40 mM? (Assume a constant temperature of 300 K)
A particular gas has a solubility in water of 1.75 mM when the pressure of the gas above water is 0.625 atm. What must the pressure of the pressure (in atm) of the gas above water be in order for the solubility to be 4.40 mM? (Assume a constant temperature of 300 K)
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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Transcribed Image Text:A particular gas has a solubility in water of 1.75 mM when the pressure of the gas
above water is 0.625 atm. What must the pressure of the pressure (in atm) of the
gas above water be in order for the solubility to be 4.40 mM? (Assume a constant
temperature of 300 K)
Expert Solution
Step 1: Define the relation between solubility and pressure
The solubility and the pressure of a gas is related by Henry’s Law.
According to Henry’s Law,
the solubility of a gas is proportional to the pressure of the gas above the solution.
S = kH × P
where S = solubility of gas
kH = Henry’s constant
P = pressure
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