Use Henry's law to determine the molar solubility of helium at a pressure of 1.2atm and 25 ∘C.
Express your answer using two significant figures.
Do you have the constant (with units please).
4.44 x 10^-4
To determine the molar solubility of helium using Henry's law, we need to use the equation:
C = kP
Where:
- C is the molar solubility of the gas in mol/L
- k is the Henry's law constant for the specific gas
- P is the partial pressure of the gas in atm
In this case, we are given the partial pressure of helium as P = 1.2 atm.
Unfortunately, the problem does not provide the specific Henry's law constant (k) for helium. The Henry's law constant varies depending on the temperature and the solvent used.
To proceed, we need the Henry's law constant for helium at the given temperature of 25 ∘C. If this information is not provided, we will need to look up the Henry's law constant for helium at this temperature.
Once we have the Henry's law constant for helium at 25 ∘C, we can use it along with the given partial pressure (P = 1.2 atm) in the equation C = kP to calculate the molar solubility (C) of helium.
Ensure to make the necessary conversions, such as converting atm to mol/L if needed, and express your final answer using two significant figures.