Use Henry’s Law to determine the molar solubility of helium at a pressure of 1.0 atm and 25 °C.

Verified step by step guidance

1. Identify the formula for Henry's Law: \( C = k_H \cdot P \), where \( C \) is the concentration (molar solubility), \( k_H \) is the Henry's Law constant, and \( P \) is the pressure.
2. Look up the Henry's Law constant \( k_H \) for helium at 25 °C. This value is typically given in units of \( \text{mol/L·atm} \).
3. Substitute the given pressure (1.0 atm) and the Henry's Law constant \( k_H \) into the Henry's Law equation.
4. Solve the equation for \( C \) to find the molar solubility of helium at the specified conditions.
5. Ensure the units are consistent and the final answer is expressed in molarity (mol/L).

Key Concepts

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 dissolved gas, kH is the Henry's Law constant, and P is the partial pressure of the gas.

Molar Solubility

Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (mol/L). It is a crucial concept in understanding how gases behave in solutions, particularly under varying pressure conditions as described by Henry's Law.

Temperature Effects on Solubility

Temperature significantly influences the solubility of gases in liquids. Generally, as temperature increases, the solubility of gases decreases due to increased kinetic energy, which allows gas molecules to escape from the liquid phase. Understanding this relationship is essential when applying Henry's Law to calculate solubility at different temperatures.