Henry's Law: Solving for Water Needed to Dissolve 1.48L of Gas

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In summary, to completely dissolve 1.48L of a gas with a Henry's law constant of 0.190M/atm at a pressure of 730torr and a temperature of 28∘C, you would need 0.2701 moles of the gas. However, to determine the amount of water needed, you would need to use the ideal gas law (PV=nRT) and account for the solubility constant and partial pressure of the gas in the solution.
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Homework Statement


How much water would be needed to completely dissolve 1.48L of the gas at a pressure of 730torrand a temperature of 28∘C? A gas has a Henry's law constant of 0.190M/atm

Homework Equations


S=kH * Pgas

The Attempt at a Solution


730 torr= .960526316 atm

S=(.190M/atm)(.960526316 atm)
S= .1825 M
.1825 mol = X = .2701 moles
1 L 1.48L

After solving that part I don't understand how to get liters of water. Maybe PV=nRT... but I tried that and I got the answer wrong.
 
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  • #2
How many moles of the gas? How many dissolved per liter of water?
 
  • #3
.2701 moles of the gas
 
  • #4
No. 1.48 L of gas at 730 torr and 28°C is not 0.27 moles.
 

What is Henry's Law?

Henry's Law is a physical law that states the amount of gas that can dissolve into a liquid is directly proportional to the partial pressure of that gas in the atmosphere above the liquid.

What is the equation for Henry's Law?

The equation for Henry's Law is: C = kP, where C is the concentration of the gas in the liquid, k is the proportionality constant, and P is the partial pressure of the gas.

How do you solve for the water needed to dissolve a specific amount of gas?

To solve for the water needed to dissolve a specific amount of gas, you can use the equation C = kP and rearrange it to solve for the concentration (C). Then, you can use the concentration to calculate the volume of water needed using the formula V = C x M, where V is the volume of water, C is the concentration, and M is the molar mass of the gas.

What is the significance of solving for water needed to dissolve gas?

Solving for the water needed to dissolve gas is important in understanding how gases interact with liquids and how they are transported in the environment. It can also help with predicting the solubility of gases in different conditions and in various industrial processes.

What factors can affect the solubility of gases in liquids according to Henry's Law?

According to Henry's Law, the solubility of gases in liquids can be affected by factors such as temperature, pressure, and the nature of the gas and liquid molecules. Higher temperatures and lower pressures can result in a higher solubility of gases in liquids, whereas the nature of the molecules can affect their ability to dissolve in a liquid.

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