Use Henry's law to determine the molar solubility of helium at a pressure of 1.5 atm and 25 degrees celsius .
this is what I know...
Sgas = kH x Pgas
so then I plugged in...
Sgas = 3.7 x 10-4 x 1.5
my answer was .055 and it is wrong.
could someone please help show me what I am doing wrong.
My first reaction is what form of Henry's law are you using? What are the units of your Henry's Law constant?
http://en.wikipedia.org/wiki/Henry%27s_law
for sgas moles/liter and pgas m/atm
redo calculations...
(3.7*10^-4)*1.5=5.7*10^-4
Ah, the molar solubility of helium, the elusive gas that just can't wait to escape your troubles and float away. Let's see if Clown Bot can bring a little laughter into this equation.
First off, kudos to you for using Henry's law! Now, let's check where you might have tripped a clown-sized shoelace.
You got the equation right: Sgas = kH x Pgas.
However, the value of kH for helium is not 3.7 x 10-4. That's actually the value for carbon dioxide. Helium's kH value is a bit different. For helium, kH is approximately 7.6 x 10-7 mol/(L x atm).
Now, plug that correct value into the equation:
Sgas = 7.6 x 10-7 x 1.5
And tada! After doing the math, you should get a molar solubility of approximately 1.14 x 10-6 mol/L for helium at a pressure of 1.5 atm and 25 degrees Celsius.
Remember, Clown Bot is here to bring laughter, not perfectly accurate answers. So, if you need more precise calculations or further assistance, it might be best to consult a human chemistry expert. Keep smiling!
To use Henry's law to determine the molar solubility of helium, we first need to know the value of the Henry's law constant (kH) for helium. Unfortunately, you did not provide that information in your question.
However, assuming a value of 3.7 x 10^-4 M/atm for the Henry's law constant (kH) of helium, we can proceed with the calculation.
The formula for Henry's law is Sgas = kH x Pgas, where Sgas is the molar solubility of the gas in solution, kH is the Henry's law constant, and Pgas is the partial pressure of the gas.
In this case, we are given a pressure of 1.5 atm and a temperature of 25 degrees Celsius. However, we need to convert the temperature to Kelvin before using it in the calculation.
To convert Celsius to Kelvin, we add 273.15 to the Celsius temperature, so 25 degrees Celsius is equal to 273.15 + 25 = 298.15 Kelvin.
Now, we can use the formula and plug in the given values:
Sgas = kH x Pgas
Sgas = (3.7 x 10^-4 M/atm) x (1.5 atm)
Sgas = 5.55 x 10^-4 M
Therefore, the molar solubility of helium at a pressure of 1.5 atm and 25 degrees Celsius would be approximately 5.55 x 10^-4 M.
If your answer of 0.055 is incorrect, it could be because you accidentally used the incorrect units for the Henry's law constant or misinterpreted the units given for the pressure. Please double-check your calculations and units to ensure their accuracy.