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If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?
- a)Argon is more soluble than CO2
- b)Argon is less soluble than CO2
- c)Argon is insoluble in water
- d)Argon and CO2 are equally soluble
Correct answer is option 'B'. Can you explain this answer?
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If, at 298 K water is the solvent, and Henry’s law constant for ...
Henry’s law is formulated asp = KH x X (mole fraction). From this, it is seen that as KH increases, mole fraction decreases in order to compensate the increase in partial pressure of the gas. Hence, higher the KH value lower is the solubility. Therefore, argon is less soluble in water than CO2 at 298 K.
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If, at 298 K water is the solvent, and Henry’s law constant for ...
's law constant for oxygen in water at 298 K is 769 torr, what is the concentration of oxygen in water at equilibrium with air at 298 K and a partial pressure of oxygen of 160 torr?
According to Henry's law, the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The equation for Henry's law is:
C = k * P
Where:
C = concentration of the gas in the liquid (in mol/L)
k = Henry's law constant (in mol/L·atm or mol/L·torr)
P = partial pressure of the gas above the liquid (in atm or torr)
Given:
k = 769 torr
P = 160 torr
Plugging in the values:
C = 769 torr * 160 torr
C = 123,040 torr^2
Therefore, the concentration of oxygen in water at equilibrium with air at 298 K and a partial pressure of oxygen of 160 torr is 123,040 torr^2.
According to Henry's law, the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The equation for Henry's law is:
C = k * P
Where:
C = concentration of the gas in the liquid (in mol/L)
k = Henry's law constant (in mol/L·atm or mol/L·torr)
P = partial pressure of the gas above the liquid (in atm or torr)
Given:
k = 769 torr
P = 160 torr
Plugging in the values:
C = 769 torr * 160 torr
C = 123,040 torr^2
Therefore, the concentration of oxygen in water at equilibrium with air at 298 K and a partial pressure of oxygen of 160 torr is 123,040 torr^2.
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If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer?
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If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer?.
If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer?.
Solutions for If, at 298 K water is the solvent, and Henry’s law constant for CO2 is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?a)Argon is more soluble than CO2b)Argon is less soluble than CO2c)Argon is insoluble in waterd)Argon and CO2 are equally solubleCorrect answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
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