Question

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 4.0 atm over the liquid at 25 °C is 1.2 x 10⁻¹ M. The Henry's law (Sg = k Pg) constant for CO₂ at this temperature is:

A) 4.5 x 10⁻³ mol / L-atm
B) 2.3 x 10⁻² mol /L-atm
C) 5.6 x 10⁻³ mol /L-atm
D) 3.0 x 10⁻² mol / L-atm

Answer 1

The Henry's law constant for CO₂ at 25 °C is 3.4 × 10-² M/atm. To find the pressure of carbon dioxide needed to maintain a concentration of 0.10 M in a can of lemon-lime soda, we can use the Henry's law equation: Sg = k Pg. Solving for P, the pressure is approximately 2.94 atm.

Step-by-step explanation:

The Henry's law constant for CO₂ in water at 25 °C is given as 3.4 × 10-² M/atm. Henry's law states that the concentration of a gas in a solution is directly proportional to its partial pressure. In this case, the pressure of carbon dioxide needed to maintain a concentration of 0.10 M in a can of lemon-lime soda can be calculated using the Henry's law equation: Sg = k Pg. Plugging in the values, we get:

0.10 M = (3.4 × 10-² M/atm) P, where P is the desired pressure of carbon dioxide.

Solving for P, we find that P = 2.94 atm. Therefore, the pressure of carbon dioxide needed to maintain a concentration of 0.10 M in a can of lemon-lime soda is approximately 2.94 atm.