Interactive Activity - Henry\'s Law Part A Click on the Run button in the activi
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Question
Interactive Activity - Henry's Law
Part A
Click on the Run button in the activity. Watch how the solubility of a gas changes as pressure is increased and then decreased during the run.
Check all that apply.
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Henrys law
S=kP
where S is the solubility of the gas, P is the partial pressure of gas over the liquid, and k is the Henrys law constant.
The Henrys law constant, k, is a value that depends on the specific gas and solvent at a specific temperature.
Part B
At a certain temperature, the solubility of N2 gas in water at 3.08atm is72.5mg of N2 gas/100 g water . Calculate the solubility of N2 gas in water, at the same temperature, if the partial pressure of N2 gas over the solution is increased from 3.08atm to 8.00atm .
Express your answer numerically to three significant figures.
188
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Correct
Part C
Calculate the solubility (in M units) of ammonia gas in water at 298 K and a partial pressure of 7.00bar . The Henrys law constant for ammonia gas at 298 K is 58.0 M/atm and 1 bar=0.9869 atm.
Express your answer in molarity to three significant figures.
Interactive Activity - Henry's Law
The solubility of a gas in a solvent changes when pressure is applied. Click here or on the image to open the activity, which illustrates the relationship between the pressure (P) and the solubility (S) of a gas. In this activity, you can see a sealed container of water and N2 gas. Click on the Run button to see the relative changes in the solubility of N2 gas in water as the pressure of the N2 gas is increased and decreased. The values of the pressure and the solubility of gas are tabulated adjacent to the Run and Reset buttons in the activity.Part A
Click on the Run button in the activity. Watch how the solubility of a gas changes as pressure is increased and then decreased during the run.
Which of the following statements correctly explain the relationship between the solubility of a gas and its pressure?Check all that apply.
As pressure is increased, the rate at which gas molecules enter the solution decreases. As pressure decreases, the concentration of gas molecules in the solution increases. The solubility of a gas decreases with a decrease in pressure. More gas molecules are soluble as pressure is increased. The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm. The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm. Fewer gas molecules are soluble at higher pressures.SubmitHintsMy AnswersGive UpReview Part
All attempts used; correct answer displayed
Henrys law
The solubility of a gas in a liquid solvent at a given temperature is directly proportional to the partial pressure of the gas over the solution. This relationship is expressed by a simple equation known as Henrys law:S=kP
where S is the solubility of the gas, P is the partial pressure of gas over the liquid, and k is the Henrys law constant.
The Henrys law constant, k, is a value that depends on the specific gas and solvent at a specific temperature.
Part B
At a certain temperature, the solubility of N2 gas in water at 3.08atm is72.5mg of N2 gas/100 g water . Calculate the solubility of N2 gas in water, at the same temperature, if the partial pressure of N2 gas over the solution is increased from 3.08atm to 8.00atm .
Express your answer numerically to three significant figures.
188
mg of N2 gas/100 g waterSubmitHintsMy AnswersGive UpReview Part
Correct
Part C
Calculate the solubility (in M units) of ammonia gas in water at 298 K and a partial pressure of 7.00bar . The Henrys law constant for ammonia gas at 298 K is 58.0 M/atm and 1 bar=0.9869 atm.
Express your answer in molarity to three significant figures.
Interactive Activity - Henry's Law The solubility of a gas in a solvent changes when pressure is applied. Click here or on the image to open the activity, which illustrates the relationship between the pressure (P) and the solubility (S) of a gas. In this activity, you can see a sealed container of water and N2 gas. Click on the Run button to see the relative changes in the solubility of N2 gas in water as the pressure of the N2 gas is increased and decreased. The values of the pressure and the solubility of gas are tabulated adjacent to the Run and Reset buttons in the activity. Part A Click on the Run button in the activity. Watch how the solubility of a gas changes as pressure is increased and then decreased during the run. Which of the following statements correctly explain the relationship between the solubility of a gas and its pressure? Check all that apply. As pressure is increased, the rate at which gas molecules enter the solution decreases. As pressure decreases, the concentration of gas molecules in the solution increases. The solubility of a gas decreases with a decrease in pressure. More gas molecules are soluble as pressure is increased. The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm. The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm. Fewer gas molecules are soluble at higher pressures. SubmitHintsMy AnswersGive UpReview Part All attempts used; correct answer displayed Henrys law The solubility of a gas in a liquid solvent at a given temperature is directly proportional to the partial pressure of the gas over the solution. This relationship is expressed by a simple equation known as Henrys law: S=kP where S is the solubility of the gas, P is the partial pressure of gas over the liquid, and k is the Henrys law constant. The Henrys law constant, k, is a value that depends on the specific gas and solvent at a specific temperature. Part B At a certain temperature, the solubility of N2 gas in water at 3.08atm is72.5mg of N2 gas/100 g water . Calculate the solubility of N2 gas in water, at the same temperature, if the partial pressure of N2 gas over the solution is increased from 3.08atm to 8.00atm . Express your answer numerically to three significant figures. 188 mg of N2 gas/100 g water SubmitHintsMy AnswersGive UpReview Part Correct Part C Calculate the solubility (in M units) of ammonia gas in water at 298 K and a partial pressure of 7.00bar . The Henrys law constant for ammonia gas at 298 K is 58.0 M/atm and 1 bar=0.9869 atm. Express your answer in molarity to three significant figures.Explanation / Answer
Part A:
Statements which are correct are -
The solubility of a gas decreases with a decrease in pressure.
More gas molecules are soluble as pressure is increased.
The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm.
The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm.
Part B:
The solubility is directly proportional to the partial pressure:
solubility at 8 atm = 72.5 * 8/3.08 mg/100 mL
= 188.3 mg/100 mL
Part C:
Cs = p x H
Cs = (7.00 x 0.9869) x 58.0
Cs = 400.7 M
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