Question

The Henry’s law constants for CO2 and O2 are 0.034 mol kg-1 bar-1 and 0.0013 mol kg-1 bar-1 respectively at 25 °C. An O2 pressure of ___ bar would be required to achieve the same solubility as 0.36 bar of CO2.

Answer 1

We know, according to Henry's law, solubility

S = k*P. (k is Henry's constant and P is partial pressure of the gas)

So, S(O2) = S(CO2). (As both solubilities are same)

--> k(O2) * P(O2) = k(CO2) * P(CO2)

--> 0.0013 * P(O2) = .034 * .36

--> P(O2) = .034 * .36/.0013

--> P(O2) = 9.42 bar.