Question

The Henry's law constant for CO2 is 3.6 ✕ 10−2 M/atm at 25°C. What pressure (in atm) of carbon dioxide is needed to maintain a CO2 concentration of 0.19 M in a can of lemon-lime soda?

Answer 1

To solve this problem we will use Henry's law. This law states that at a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure exerted by that gas on the liquid. Mathematically it is formulated as follows:

$C = K_H*P$

Where,

$K_H$ = Henry's constant for C02 at 25°C is equal to $3.6*10^{-2}M/atm$

C = Gas concentration is 0.19M

Replacing we have,

$0.19 M = (3.6*10^-2 M/atm)*P$

$P = 5.277 atm$

Therefore the pressure of carbon dioxide is 5.277 atm