Chapter 10, Problem 29QAP

A carbonated beverage is made by saturating water with carbon dioxide at 0°C and a pressure of 3.0 atm. The bottle is then opened at room temperature (25°C), and comes to equilibrium with air in the room containing ${\text{CO}}_2\left(P_{{\text{CO}}_2}=1.0\times {10}^{-3}\text{M}/\text{atm}\right)$. The Henry's law constant for the solubility of CO₂ in water is 0.0769 M/atm at 0°C and 0.0313 M/atm at 25°C.

(a) What is the concentration of carbon dioxide in the bottle before it is opened?

(b) What is the concentration of carbon dioxide in the bottle after it has been opened and come to equilibrium with the air?