Use Henry's law to determine the molar solubility of helium at a pressure of 1.5 atm and 25deg C.
http://answers.yahoo.com/question/index?qid=20100418160251AAxjhIE
To use Henry's law to determine the molar solubility of helium, we need to know its Henry's law constant and the partial pressure of helium.
Henry's law states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. Mathematically, it can be expressed as:
C = k * P
where C is the concentration of the gas in the liquid, k is the Henry's law constant, and P is the partial pressure of the gas.
However, before we can proceed, we need to convert the given pressure from atm to units that are consistent with the units used for the Henry's law constant. Normally, the Henry's law constant is given with units in M/atm or mol/L/atm.
Let's assume the Henry's law constant for helium is given as k = 3.34 x 10^-4 mol/L/atm at 25°C.
Now, we can substitute the given values into the equation and solve for the molar solubility (C) of helium:
C = k * P
C = (3.34 x 10^-4 mol/L/atm) * (1.5 atm)
C = 5.01 x 10^-4 mol/L
Therefore, the molar solubility of helium at a pressure of 1.5 atm and 25°C is approximately 5.01 x 10^-4 mol/L.