The Henry’s law constant for helium gas in water at 30 °C is 3.7 * 10^-4 M/atm and the constant for N2 at 30 °C is 6.0 * 10^-4 M/atm. If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas.

Verified step by step guidance

Step 1: Understand Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is given by S = kH * P, where S is the solubility, kH is the Henry's law constant, and P is the partial pressure of the gas.

Step 2: Identify the given values for helium: the Henry's law constant (kH) is 3.7 * 10^-4 M/atm and the partial pressure (P) is 1.5 atm.

Step 3: Calculate the solubility of helium using the formula S = kH * P. Substitute the given values for helium into the equation.

Step 4: Identify the given values for nitrogen (N2): the Henry's law constant (kH) is 6.0 * 10^-4 M/atm and the partial pressure (P) is 1.5 atm.

Step 5: Calculate the solubility of nitrogen using the formula S = kH * P. Substitute the given values for nitrogen into the equation.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This relationship can be expressed mathematically as C = kH * P, where C is the concentration of the gas in the liquid, kH is the Henry's law constant, and P is the partial pressure of the gas.

Solubility

Solubility refers to the maximum amount of a substance that can dissolve in a given quantity of solvent at a specific temperature and pressure. In the context of gases, solubility is influenced by factors such as temperature, pressure, and the nature of the gas and solvent, which can affect how much gas can be dissolved in the liquid.

Units of Concentration

In this context, the solubility of gases is expressed in molarity (M), which is moles of solute per liter of solution. Understanding how to convert between different units of concentration and how to apply them in calculations is essential for determining the solubility of gases using Henry's Law.

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Indicate whether each statement is true or false: (c) As you cool a saturated solution from high temperature to low temperature, solids start to crystallize out of solution if you achieve a supersaturated solution.

Textbook Question

Indicate whether each statement is true or false: (d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the solution even more concentrated.

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Textbook Question

Indicate whether each statement is true or false: (c) The solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised.

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Open Question

The partial pressure of O2 in air at sea level is 0.21 atm. Using the data in Table 13.1, together with Henry’s law, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 °C and an atmospheric pressure of 650 torr.

Textbook Question

(a) Calculate the mass percentage of Na₂SO₄ in a solution containing 10.6 g of Na₂SO₄ in 483 g of water.

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Open Question

(b) An ore contains 2.86 g of silver per ton of ore. What is the concentration of silver in ppm?