The henry's law constant (k) for carbon monoxide in water at 25 degree C is 9.71 * 10 ^-4 mol/(L*atm)
How many moles of CO will dissolve in 1.00 L of water if the partial pressure of CO is 2.75 atm?
waht pressure of carbon dioxide is required to keep the carbon dioxide concentration in a bottle of club soda at .12 M at 25 degrees C?
Info: Kh for Co2 at 25 degrees C = 3.4 * 10^-2 M/atm
Answer to that is 3.5 atm
The Attempt at a Solution
s(g) = Kh * Pg
Since i don't have the Molarity i have no idea what to do.
M = moles solute ( i dont know if the water or CO is the solvent or solute)
divided by L solution
(9.71*10^-4mol/L*atm)(2.75 atm) = 2.67 *10^-3 mol/L
2.67*10^-3 mol/L * 1.00 L = 2.67*10^-3 mol
i have no idea what to do from there