The solubility of CO2 in water is 3.2 x 10^2 M at 25 C and 1 atm pressure. What is the Henry's Law constant for CO2 in mol/(L atm)?
c=kP 0.25= kP
p=kc
p/k=kc/k
=Px 1/k
Please help!
To find the Henry's Law constant for CO2 in mol/(L atm), we need to rearrange the equation c = kP, where c is the solubility of CO2 in water in M (mol/L), k is the Henry's Law constant in mol/(L atm), and P is the partial pressure of CO2 in atm.
We are given the solubility of CO2 (c) as 3.2 x 10^2 M at 1 atm pressure. Let's substitute these values into the equation:
3.2 x 10^2 M = k x 1 atm
To find the Henry's Law constant (k), we need to rearrange this equation:
k = c/P
Substituting the given values:
k = (3.2 x 10^2 M) / (1 atm)
k = 3.2 x 10^2 M/atm
Therefore, the Henry's Law constant for CO2 is 3.2 x 10^2 mol/(L atm).