Question

the concentration of co2 in a soft drink bottle with a partial pressure of co2 of 6.5 atm over the liquid at 29 C is 2.2 x 10^-1 M. The Henry's law constant for CO2 at this temperatur is

Answer 1

Answer: The Henry's constant for carbon dioxide is
`3.38* 10^(-2)mol/L.atm`

Step-by-step explanation:

To calculate the molar solubility, we use the equation given by Henry's law, which is:

`C_(CO_2)=K_H* p_(CO_2)`

where,

`K_H` = Henry's constant = ?

`C_(CO_2)` = molar solubility of carbon dioxide gas =
`2.2* 10^(-1)mol/L`

`p_(CO_2)` = partial pressure of carbon dioxide gas = 6.5 atm

Putting values in above equation, we get:

`2.2* 10^(-1)mol/L=K_H* 6.5atm\\\\K_H=(2.2* 10^(-1)mol/L)/(6.5atm)=3.38* 10^(-2)mol/L.atm`

Hence, the Henry's constant for carbon dioxide is
`3.38* 10^(-2)mol/L.atm`