How Many Moles of CO Dissolve in Water According to Henry's Law?

[imxaxpunk]

Homework Statement

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?

Homework Equations

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 don't 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

 

[nate808]

To find the number of moles of CO that will dissolve in 1.00 L of water, we can use the Henry's law equation:
s(g) = k * Pg
where s(g) is the solubility of CO in water, k is the Henry's law constant, and Pg is the partial pressure of CO.
In this case, we have:
s(g) = (9.71 * 10^-4 mol/(L*atm)) * (2.75 atm) = 2.67 * 10^-3 mol/L
This means that 2.67 * 10^-3 moles of CO will dissolve in 1.00 L of water.
As for your second question about the pressure of carbon dioxide needed to maintain a concentration of 0.12 M in club soda, we can use a similar equation:
s(g) = k * Pg
where s(g) is the solubility of CO2 in water, k is the Henry's law constant, and Pg is the partial pressure of CO2.
We can rearrange this equation to solve for Pg:
Pg = s(g)/k
Plugging in the given values, we have:
Pg = (0.12 M)/(3.4 * 10^-2 M/atm) = 3.5 atm
Therefore, a pressure of 3.5 atm of CO2 is needed to maintain a concentration of 0.12 M in club soda at 25 degrees C.
I hope this helps!