Question

Sealed containers of fizzy drinks contain dissolved carbon dioxide. The dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container.

Find partial pressure of CO2 gas in 355 ml can of fizzy drink at 25C if the concentration of CO2 in the fizzy drink 0.1 M. Given that Henry’s law constant for CO2 is 3.3 x 10-2 M atm-1.

What mass of CO2 is dissolved in a 355 ml can of fizzy drink when it is stored at 25C.

Answer 1

3 atm

1.6 g

Step-by-step explanation:

Step 1: Given data

• Volume of the solution (V): 355 mL

• Concentration of the solution (C): 0.1 M

• Henry’s law constant for CO₂ (k): 3.3 × 10⁻² M atm⁻¹.

Step 2: Find partial pressure (P) of CO₂ gas

We will use Henry's law.

C = k × P

P = C / k

P = 0.1 M / 3.3 × 10⁻² M atm⁻¹

P = 3 atm

Step 3: Calculate the mass of CO₂ gas

The molar mass of carbon dioxide is 44.01 g/mol.

0.355 L × 0.1 mol/L × 44.01 g/mol = 1.6 g