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).